Answer:
0.779
Explanation:
Determine the molecular weight of the hydrocarbon. We know that its vapor density is 29, which means that one mole of the hydrocarbon has a mass of 29 grams. Therefore, the molecular weight of the hydrocarbon is 29 g/mol.
Calculate the number of moles of the hydrocarbon. We can use the formula:
moles = mass / molecular weight
Substituting the values, we get:
moles = 29 g / 29 g/mol = 1 mol
Therefore, we have one mole of the hydrocarbon.
Write the balanced chemical equation for the combustion of the hydrocarbon in oxygen. The general equation is:
hydrocarbon + oxygen → carbon dioxide + water
For one mole of the hydrocarbon, we need one mole of oxygen to completely burn it. The balanced equation is:
CnHm + (n+m/4) O2 → n CO2 + m/2 H2O
Calculate the volume of carbon dioxide produced. We know that 1 mole of any gas at STP occupies 22.4 L. Therefore, one mole of carbon dioxide occupies 22.4 L. The volume of 448 ml of carbon dioxide at STP can be converted to liters:
448 ml = 0.448 L
The number of moles of carbon dioxide produced can be calculated using the ideal gas law:
PV = nRT
where P is the pressure (1 atm), V is the volume (0.448 L), n is the number of moles, R is the gas constant (0.0821 L atm/mol K), and T is the temperature (273 K). Substituting the values, we get:
n = PV/RT = (1 atm x 0.448 L) / (0.0821 L atm/mol K x 273 K) = 0.0177 mol
Therefore, 0.0177 moles of carbon dioxide are produced.
Calculate the mass of carbon dioxide produced. We can use the formula:
mass = moles x molecular weight
The molecular weight of carbon dioxide is 44 g/mol. Substituting the values, we get:
mass = 0.0177 mol x 44 g/mol = 0.779 g
Therefore, the mass of carbon dioxide produced is 0.779 grams.
Write the following chemical reactions and balance:
Potassium reacts with sodium oxide to produce potassium oxide and sodium
The chemical reaction between potassium and sodium oxide results in the formation of potassium oxide and sodium. The balanced equation for this reaction is:
2K + Na₂O -> K₂O + 2Na
This reaction is an example of a displacement reaction, where a more reactive element (potassium) displaces a less reactive element (sodium) from its compound (sodium oxide). The displacement occurs because potassium has a greater tendency to lose electrons and form cations compared to sodium.
Potassium oxide is an important chemical compound with many industrial applications, including in the production of glass, ceramics, and fertilizers. It is also used as a drying agent and catalyst in organic reactions.
Sodium, on the other hand, is a highly reactive metal that is commonly found in compounds such as sodium chloride (table salt) and sodium hydroxide (lye). It is an essential element for many biological processes, including nerve and muscle function.
Overall, this chemical reaction between potassium and sodium oxide is important because it highlights the reactivity of these elements and the formation of useful compounds such as potassium oxide. It also emphasizes the importance of balancing chemical equations to ensure that the reactants and products are in the correct proportions.
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flew by Mercury in 1974; took photographs, temperature readings, and gathered atmosphere information; sent the information back to earth through radio waves
In 1974, the 1973-launched Mariner 10 spacecraft made history by flying by Mercury for the first time.
What is spacecraft?A vehicle made specifically for space travel is a spaceship. It can encompass both spacecraft made for study, observation, and the deployment of satellites and other payloads as well as those made for human exploration, communication, and transportation. They typically consist of a propulsion system, navigation system, communications system, and numerous payloads, among other things. Typically, a spacecraft needs a launch vehicle to get off the ground and a re-entry mechanism to land safely.
It recorded temperature readings, snapped pictures, and gathered data on the planet's atmosphere during its flyby. Then, radio waves were used to transmit all of this data back to Earth. The mission was a great success and revealed a tonne of fresh Mercury-related data.
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The complete question is,
passed past Mercury in 1974, taking pictures, measuring temperatures, and gathering data on the atmosphere before radio-transmitting the data back to Earth.
What is the strongest type of intermolecular forces present between the hydrocarbon chains of neighboring stearic acid molecules?
The strongest type of intermolecular forces present between the hydrocarbon chains of neighboring stearic acid molecules is van der Waals forces, specifically London dispersion forces.
These forces arise due to temporary fluctuations in electron distribution, causing momentary dipoles that attract adjacent molecules.
Stearic acid is a long-chain fatty acid consisting of a hydrocarbon chain (nonpolar) and a carboxylic acid functional group (polar). The hydrocarbon chains in stearic acid are composed of carbon and hydrogen atoms, resulting in a relatively nonpolar nature.
London dispersion forces, also known as instantaneous dipole-induced dipole interactions, are intermolecular forces that occur between all molecules, including nonpolar molecules like stearic acid.
These forces arise due to temporary fluctuations in the electron distribution around atoms or molecules, leading to the formation of temporary dipoles.
In the case of stearic acid, the temporary dipole moment that arises in one molecule induces a corresponding dipole in the neighboring molecule, creating an attractive force between them.
These temporary dipoles result from the uneven distribution of electrons at any given moment, leading to the establishment of temporary positive and negative charges.
The strength of London dispersion forces depends on factors such as the size of the molecules involved and the ease of electron movement within them.
In the hydrocarbon chains of stearic acid, the presence of a large number of carbon atoms increases the surface area available for intermolecular interactions, making the London dispersion forces relatively stronger.
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An ethanol plant distills alcohol from corn. The distiller processes 2. 0 t/h of feed containing 15% alcohol and 82% water; the rest is inert material. The bottoms (waste) produced is 85% of the feed and contains 94% water, 3. 5% inert material, and 2. 5% alcohol. The vapor (product) from the top of the distiller is passed through a condenser and cooled to produce the final product. Determine the rate of production of the final product and its composition
The rate of production of the final product is 0.3 t/h, and the composition of the final product is approximately 12.5% alcohol and 12% water, with no inert material present.
In an ethanol plant, the distillation process separates alcohol from corn. With a feed rate of 2.0 tons per hour, the bottoms waste contains 85% of the feed, while the final product is obtained from condensing and cooling the vapor.
To determine the rate of production of the final product and its composition, we need to calculate the mass flow rate of the final product and the composition of the final product.
Given:
Feed rate = 2.0 t/h
Composition of feed:
Alcohol: 15%
Water: 82%
Inert material: (100% - 15% - 82%) = 3%
Bottoms composition:
Water: 94%
Inert material: 3.5%
Alcohol: 2.5%
To calculate the rate of production of the final product, we need to subtract the mass of bottoms produced from the feed rate:
Rate of production of the final product = Feed rate - Mass of bottoms
Mass of bottoms = Feed rate × Bottoms composition = 2.0 t/h × 85% = 1.7 t/h
Rate of production of the final product = 2.0 t/h - 1.7 t/h = 0.3 t/h
Therefore, the rate of production of the final product is 0.3 tons per hour.
To calculate the composition of the final product, we need to consider the remaining components after removing the bottoms:
Composition of final product:
Alcohol: 15% - 2.5% = 12.5%
Water: 82% - 94% = 12%
Inert material: 3% - 3.5% = -0.5% (Assuming a negative value means there is no inert material remaining)
Therefore, the composition of the final product is approximately:
Alcohol: 12.5%
Water: 12%
No inert material
Please note that the negative value for the inert material indicates that there is no inert material present in the final product.
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1. Hydrogen + oxygen yields water
Label what type of reaction (synthesis, decomposition, single replacement, double replacement or combustion)
Write the balanced chemical equation
How much water could you get if you started with 250. 0 grams of hydrogen?
How much water could you get if you started with 250. 0 grams of oxygen?
Which is the limiting reactant?
Labeling the type of reaction:
This is a synthesis reaction because two elements (hydrogen and oxygen) are combining to form a compound (water).
Writing the balanced chemical equation:
2H2 + O2 → 2H2O
Determining how much water can be produced from 250.0 grams of hydrogen:
We need to use stoichiometry to calculate the amount of water produced from a given amount of hydrogen. The balanced chemical equation tells us that 2 moles of hydrogen reacts with 1 mole of oxygen to produce 2 moles of water.
First, let's convert 250.0 grams of hydrogen to moles:
moles of H2 = mass of H2 / molar mass of H2
= 250.0 g / 2.016 g/mol
= 124.01 mol
Using the mole ratio from the balanced chemical equation, we can calculate the moles of water produced:
moles of H2O = (2 moles of H2 / 2) × (1 mole of H2O / 2 moles of H2) × 124.01 moles of H2
= 62.005 moles of H2O
Finally, we can convert moles of water to grams:
mass of H2O = moles of H2O × molar mass of H2O
= 62.005 mol × 18.015 g/mol
= 1115.9 g
Therefore, 250.0 grams of hydrogen can produce 1115.9 grams of water.
Determining how much water can be produced from 250.0 grams of oxygen:
We need to use stoichiometry again, but this time we'll start with the mass of oxygen.
From the balanced chemical equation, we know that 1 mole of oxygen reacts with 2 moles of hydrogen to produce 2 moles of water.
First, let's convert 250.0 grams of oxygen to moles:
moles of O2 = mass of O2 / molar mass of O2
= 250.0 g / 31.999 g/mol
= 7.813 moles
Using the mole ratio from the balanced chemical equation, we can calculate the moles of water produced:
moles of H2O = (1 mole of O2 / 2) × (2 moles of H2O / 1 mole of O2) × 7.813 moles of O2
= 7.813 moles of H2O
Finally, we can convert moles of water to grams:
mass of H2O = moles of H2O × molar mass of H2O
= 7.813 mol × 18.015 g/mol
= 140.65 g
Therefore, 250.0 grams of oxygen can produce 140.65 grams of water.
Determining the limiting reactant:
To determine the limiting reactant, we need to compare the amount of product that can be produced from each reactant. The reactant that produces the smaller amount of product is the limiting reactant.
From our calculations above, we found that 250.0 grams of hydrogen can produce 1115.9 grams of water, and 250.0 grams of oxygen can produce 140.65 grams of water. Therefore, the limiting reactant is oxygen because it produces less water than hydrogen.
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The volume of a sample of hydrogen gas at 0. 997 atm is 5. 00 L. What will be the new volume if the pressure is decreased to 0. 977 atm?
The new volume of the hydrogen gas is 5.12 L when the pressure is decreased to 0.977 atm.
The relationship between pressure and volume is described by Boyle's Law, which states that when the pressure of a gas decreases, its volume increases proportionally, and vice versa. In other words, the pressure and volume of a gas are inversely proportional, assuming temperature and amount of gas remain constant.
In this case, the initial pressure of the hydrogen gas is 0.997 atm, and its initial volume is 5.00 L. If the pressure is decreased to 0.977 atm, we can use Boyle's Law to calculate the new volume:
P1V1 = P2V2
Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the new pressure and volume.
Substituting the given values, we get:
(0.997 atm)(5.00 L) = (0.977 atm)(V2)
Solving for V2, we get:
V2 = (0.997 atm)(5.00 L) / (0.977 atm)
V2 = 5.12 L
Therefore, the new volume of the hydrogen gas is 5.12 L when the pressure is decreased to 0.977 atm.
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A gas occupies 37. 5 mL at 102. 3 kPa. At 27. 5 mL, what will the pressure be?
A gas has an initial volume of 37.5 mL at a pressure of 102.3 kPa. When the volume decreases to 27.5 mL, the pressure increases to 139.8 kPa.
This question can be solved using Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at a constant temperature. Therefore, we can use the equation P1V1 = P2V2, where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume.
Substituting the given values into the equation, we get:
P1V1 = P2V2
(102.3 kPa)(37.5 mL) = P2(27.5 mL)
Solving for P2, we get:
P2 = (102.3 kPa)(37.5 mL) / 27.5 mL
P2 = 139.32 kPa
Therefore, the pressure of the gas when its volume is 27.5 mL will be 139.32 kPa.
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Methane (CH4) is a common fuel to heat homes in the winter. What is the molar enthalpy of combustion of methane? Assume this combustion occurs entirely in the gas phase. Bond Enthalpies(in kJ molâ1):CâC: 347 CâH: 413 HâH:432 OâH: 467 C=C: 614C=O: 745O=O: 498
A)â710kJ molâ1
B)â297 kJmolâ1
C)â1843 kJmolâ
1D)+792 kJmolâ1
E)+567 kJmol
The molar enthalpy of combustion of methane in the gas phase is approximately -1360 kJ/mol, which is closest to -297 kJ/mol. The correct option is B.
To determine the molar enthalpy of combustion of methane, we need to use the bond enthalpies provided to calculate the energy released when the bonds in methane are broken and new bonds are formed in the combustion reaction.
The balanced chemical equation for the combustion of methane is:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
Breaking the bonds in methane requires energy while forming the new bonds in carbon dioxide and water releases energy. The molar enthalpy of combustion is the net energy released per mole of methane combusted.
Using the bond enthalpies given, we can calculate the energy required to break the bonds in methane:
4C-H bonds x 413 kJ/mol = 1652 kJ/mol
1C-C bond x 347 kJ/mol = 347 kJ/mol
Total energy required to break bonds in methane = 1652 kJ/mol + 347 kJ/mol = 1999 kJ/mol
Next, we can calculate the energy released by forming the new bonds in carbon dioxide and water:
2C=O bonds x 745 kJ/mol = 1490 kJ/mol
4O-H bonds x 467 kJ/mol = 1868 kJ/mol
Total energy released by forming new bonds = 1490 kJ/mol + 1868 kJ/mol = 3358 kJ/mol
The net energy released in the combustion of methane is the energy released by forming new bonds minus the energy required to break the old bonds:
Net energy released = 3358 kJ/mol - 1999 kJ/mol = 1359 kJ/mol
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What volume (in litres) of 0. 200 M NaOH is required to neutralize 22. 3 mL of 0. 152 M HCl?
To solve this problem, we can use the following equation:
Moles of acid = Moles of base
where "acid" refers to the HCl and "base" refers to the NaOH.
First, let's calculate the moles of HCl:
moles of HCl = concentration of HCl × volume of HCl
= 0.152 mol/L × 0.0223 L
= 0.0033856 mol
Next, let's calculate the volume of NaOH required to neutralize the HCl:
moles of NaOH = moles of HCl
volume of NaOH = moles of NaOH / concentration of NaOH
We know the concentration of NaOH (0.200 M), so let's substitute in the values:
moles of NaOH = 0.0033856 mol
volume of NaOH = 0.0033856 mol / 0.200 mol/L
= 0.016928 L
= 16.928 mL (rounded to three decimal places)
Therefore, 16.928 mL of 0.200 M NaOH is required to neutralize 22.3 mL of 0.152 M HCl.
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The exhaust gas coming from a coal-burning furnace (flue gas) usually contains sulfur in the form of so2, and when the gas is discharged into the atmosphere (which sometimes hap- pens), the so2 can eventually react with oxygen and water to form sulfuric acid (h2so4 ), hence, acid rain. the reaction is
The reaction of sulfur dioxide (SO₂) with oxygen and water to form sulfuric acid (H₂SO₄) is responsible for acid rain. The reaction is: SO₂(g) + O₂(g) + H₂O(l) -> H₂SO₄(aq).
When flue gas from a coal-burning furnace is discharged into the atmosphere, it contains sulfur dioxide (SO₂) as one of its components. SO₂ can react with oxygen and water in the atmosphere to form sulfuric acid (H₂SO₄), which is a strong acid that can cause harm to the environment. Sulfuric acid is one of the main components of acid rain, which can damage crops, forests, and bodies of water, as well as erode buildings and other structures.
Acid rain can also be harmful to human health, as it can cause respiratory problems and other illnesses. Therefore, it is important to control the emissions of SO₂ from coal-burning furnaces and other sources to reduce the formation of sulfuric acid and the occurrence of acid rain.
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Micheal has an infection in his sinuses and lungs, but has no sick
time, so goes to work anyway. He is coughing and sneezing the
whole shift and only remembers to cover his nose and mouth about
half the time. Which link represents the break in the chain of
infection in this scenario, placing you at risk of contracting the
infection?
f
Select one:
a.
Reservoir
b.
Infectious agerte
C.
Port of exit
d.
Port of entry
The link that represents the break in the chain of infection in this scenario, placing you at risk of contracting the infection is the Port of entry.
The worker is coughing and sneezing without covering his nose and mouth, which allows the infectious agents to enter the body of others nearby. The Port of entry is the point at which the infectious agents enter the susceptible host, and in this case, it is through inhalation of respiratory droplets from the sick worker. This highlights the importance of proper hygiene practices, such as covering your nose and mouth when coughing or sneezing, to prevent the spread of infectious diseases in the workplace.
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The evaporation heat of mercury is 296 kJ/ kg. Calculate how much heat needs to be provided to change 50 g of this substance into vapour at its boiling point
To calculate the amount of heat required to change 50 g of mercury into vapor at its boiling point, we need to use the following formula:
Q = m * H_vap
where Q is the amount of heat required, m is the mass of the substance, and H_vap is the heat of vaporization.
We are given that the heat of vaporization of mercury is 296 kJ/kg. To use this value, we need to convert the mass of mercury to kilograms:
m = 50 g = 0.05 kg
Now we can use the formula to calculate the amount of heat required:
Q = 0.05 kg * 296 kJ/kg = 14.8 kJ
Therefore, 14.8 kJ of heat needs to be provided to change 50 g of mercury into vapor at its boiling point.
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Counting Atoms and Elements in a Chemical Formula (8. 5D)
For example, the chemical formula for water is H₂O. This tells us that there are two hydrogen atoms (H) and one oxygen atom (O) in each molecule of water. To count the number of atoms in a chemical formula, we can use the subscripts (the numbers that come after each element symbol) to determine how many atoms of each element are present. For example, in the chemical formula NaCl (which represents salt), there is one sodium (Na) atom and one chlorine (Cl) atom in each molecule.
Let us discuss this in detail. To count atoms and elements in a chemical formula, you need to understand the following terms:
- Atoms: The basic unit of a chemical element, consisting of protons, neutrons, and electrons.
- Elements: A substance that cannot be broken down into simpler substances, consisting of only one type of atom.
- Chemical Formula: A representation of a substance using symbols for its constituent elements and numbers to indicate the ratio of atoms in the compound.
Now, let's count the atoms and elements in a given chemical formula, for example, H₂O (water):
1. Identify the elements in the formula: In this case, we have two elements - Hydrogen (H) and Oxygen (O).
2. Count the atoms of each element: The subscript number next to each element symbol indicates the number of atoms of that element in the compound. For Hydrogen (H), the subscript is 2, meaning there are 2 Hydrogen atoms. For Oxygen (O), there is no subscript, which means there is only 1 Oxygen atom (when no subscript is present, it is understood to be 1).
So, in the chemical formula H₂O, there are 2 Hydrogen atoms and 1 Oxygen atom, for a total of 3 atoms.
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A 4.1 g sample of gold (specific heat capacity = 0.130 J/g °C) is heated using 52.2 J of energy. If the original temperature of the gold is 25.0°C, what is its final temperature?
To solve this problem, we can use the formula:
q = m*c*ΔT, where q is the amount of heat energy absorbed by the gold, m is the mass of the gold, c is the specific heat capacity of gold, and ΔT is the change in temperature of the gold.
We are given the mass of gold (m = 4.1 g), the specific heat capacity of gold (c = 0.130 J/g °C), and the amount of energy used to heat the gold (q = 52.2 J). We are asked to find the final temperature of the gold (ΔT).
Rearranging the formula, we get:
ΔT = q/(m*c)
Substituting the values we know, we get:
ΔT = 52.2 J / (4.1 g * 0.130 J/g °C)
ΔT = 98.92 °C
This is the change in temperature of the gold. To find the final temperature, we add this to the original temperature of 25.0°C:
Final temperature = 25.0°C + 98.92°C
Final temperature = 123.92°C
Therefore, the final temperature of the gold is 123.1°C.
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Help plssssssssss
what are the condensed formula of the following alkyl
no.of alkyles condensed formula
carbons
1 methyl
2 ethyl
3 propyl
4 butyl
5 pentyl
6 hexyl
7 heptyl
8 oktyl
9 nonyl
10 dekyl
11 undekyl
12. dodekyl
Here are the condensed formulas for each alkyl group, with the number of number of carbons:
1. Methyl (1 carbon): CH3-
2. Ethyl (2 carbons): CH3CH2-
3. Propyl (3 carbons): CH3CH2CH2-
4. Butyl (4 carbons): CH3(CH2)3-
5. Pentyl (5 carbons): CH3(CH2)4-
6. Hexyl (6 carbons): CH3(CH2)5-
7. Heptyl (7 carbons): CH3(CH2)6-
8. Octyl (8 carbons): CH3(CH2)7-
9. Nonyl (9 carbons): CH3(CH2)8-
10. Decyl (10 carbons): CH3(CH2)9-
11. Undecyl (11 carbons): CH3(CH2)10-
12. Dodecyl (12 carbons): CH3(CH2)11-
These formulas represent alkyl groups, which are fragments of alkane molecules with one hydrogen atom removed. They can attach to other molecules and form various organic compounds.
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Calculate the mass of iron that releases 2432 J of energy as its temperture rises from 25. 0 degrees * C to 87. 0 degrees * C. (The specific heat of iron is 0. 448 J/g^ C)
To solve this problem, we can use the formula:
q = m * c * ΔT
where q is the heat energy absorbed or released, m is the mass of the substance, c is the specific heat capacity of the substance, and ΔT is the change in temperature.
We know that the heat energy released by the iron is 2432 J, the specific heat capacity of iron is 0.448 J/g°C, the initial temperature of the iron is 25.0°C, and the final temperature of the iron is 87.0°C.
The mass of iron that releases 2432 J of energy as its temperature rises from 25.0°C to 87.0°C is 96.2 g.
Substituting the values in the formula, we get:
2432 J = m * 0.448 J/g°C * (87.0°C - 25.0°C)
Simplifying the equation, we get:
m = 2432 J / (0.448 J/g°C * 62.0°C)
m = 96.2 g
Therefore, the mass of iron that releases 2432 J of energy as its temperature rises from 25.0°C to 87.0°C is 96.2 g.
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`Name:
Date:
Properties of Matter - Crunch time Review
1. If two objects balance like the ones shown below, what must be true?
A. Object A has more mass than object B.
Both objects have the same mass.
C. Object A has more volume than object B.
D. Both objects have the same volume.
Answer:
d
Explanation:
because i did it
you need to make an aqueous solution of 0.172 m iron(ii) nitrate for an experiment in lab, using a 250 ml volumetric flask. how much solid iron(ii) nitrate should you add?
We need to add 7.7 g of solid iron(II) nitrate to make a 0.172 M solution in 250 mL volumetric flask.
First, we can use molarity and volume of solution to find the number of moles of iron(II) nitrate needed:
moles of [tex]Fe(NO_3)_2[/tex]= Molarity × Volume in liters
moles of [tex]Fe(NO_3)_2[/tex] = 0.172 mol/L × 0.250 L = 0.043 mol
Next, we can use the molar mass of iron(II) nitrate to find the mass of the solid that needs to be added:
mass of [tex]Fe(NO_3)_2[/tex] = moles of [tex]Fe(NO_3)_2[/tex] × molar mass of [tex]Fe(NO_3)_2[/tex]
mass of [tex]Fe(NO_3)_2[/tex]= 0.043 mol × (55.85 g/mol + 2 × 14.01 g/mol + 6 × 16.00 g/mol)
mass of [tex]Fe(NO_3)_2[/tex]= 0.043 mol × 179.86 g/mol = 7.7 g
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7. 50 mL of an acetic acid (CH3CO2H, 60. 05 g/mole) stock solution was added to an analyte flask, along with 15 mL of water. 14. 36 mL of 0. 0915 M NaOH titrant was required to titrate the analyte solution to the endpoint. Calculate the concentration of the stock solution. Watch significant figures
The concentration of the acetic acid stock solution is 0.026259 M, considering significant figures.
To solve this problem, we first need to write out the balanced chemical equation for the reaction between acetic acid (CH₃CO₂H) and sodium hydroxide (NaOH):
CH₃CO₂H + NaOH → CH₃CO₂Na + H₂O
We can see from this equation that the stoichiometry of the reaction is 1:1 - that is, one mole of acetic acid reacts with one mole of NaOH. We also know that the volume of the analyte solution is 50 mL + 15 mL = 65 mL.
Next, we need to use the volume and concentration of the NaOH titrant to calculate the number of moles of NaOH that were added to the analyte solution:
V1 = 14.36 mL = 0.01436 L (convert mL to L)
C1 = 0.0915 M
n(NaOH) = V1 x C1 = 0.01436 L x 0.0915 mol/L = 0.00131294 mol
Since the stoichiometry of the reaction is 1:1, we know that this is also the number of moles of acetic acid that were present in the analyte solution. We can use this information to calculate the concentration of the stock solution:
n(CH₃CO₂H) = n(NaOH) = 0.00131294 mol
V2 = 50 mL = 0.05 L (convert mL to L)
M = n/V = 0.00131294 mol / 0.05 L = 0.026259 M
So the concentration of the acetic acid stock solution is 0.026259 M.
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Would you expect a C8 molecule to boil at a higher or lower temperature than a C24 molecule?
I would expect a C24 molecule to boil at a higher temperature than a C8 molecule.
What is the temperature about?The boiling point of a molecule depends on the strength of intermolecular forces between the individual molecules. Intermolecular forces are forces that exist between molecules and they include dipole-dipole forces, hydrogen bonding, London dispersion forces, and ion-dipole forces.
This is because the boiling point of a molecule is directly related to its size and the strength of its intermolecular forces. A larger molecule such as C24 has more electrons and a larger surface area, which results in stronger intermolecular forces such as London dispersion forces.
These stronger forces require more energy to be overcome and thus result in a higher boiling point. In contrast, a smaller molecule such as C8 has weaker intermolecular forces and requires less energy to overcome them, resulting in a lower boiling point.
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A mixture of 100 mol containing 60 mol % n-pentane and 40 mol% n-heptane is vaporized at 101. 32 kpa abs pressure until 40 mol of vapor and 60 mol of liquid in equilibrium with each other are produced. this occurs in a single-state system, and the vapor and liquid are kept in contact with each other until vaporization is complete.
required:
calculate the composition of the vapor and the liquid
The composition of the vapor phase is 25.2 mol% n-pentane and 4.8 mol% n-heptane, and the composition of the liquid phase is 67.4 mol% n-pentane and 32.6 mol% n-heptane.
To calculate the composition of the vapor and the liquid, we can use the Raoult's law equation:
P_A = X_A * P^0_A
where P_A is the partial pressure of component A, X_A is the mole fraction of component A, and P^0_A is the vapor pressure of pure component A.
For n-pentane, the vapor pressure at 101.32 kPa abs is 42.5 kPa abs, and for n-heptane, it is 12.1 kPa abs. Using the given mole fractions, we can calculate the partial pressures of each component in the mixture:
P_n-pentane = 0.6 * 42.5 = 25.5 kPa abs
P_n-heptane = 0.4 * 12.1 = 4.84 kPa abs
Next, we can use the total pressure of the system (101.32 kPa abs) and the partial pressures to calculate the mole fractions of each component in the vapor and the liquid phases:
For the vapor phase:
X_n-pentane = P_n-pentane / 101.32 = 0.252
X_n-heptane = P_n-heptane / 101.32 = 0.048
For the liquid phase:
Y_n-pentane = (0.6 - 0.4 * X_n-heptane) / (1 - X_n-heptane) = 0.674
Y_n-heptane = 0.326
Therefore, the composition of the vapor phase is 25.2 mol% n-pentane and 4.8 mol% n-heptane, and the composition of the liquid phase is 67.4 mol% n-pentane and 32.6 mol% n-heptane.
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Two students in a chemistry lab start a particular lab with 1. 23 g of aluminum. They react it with excess sulfuric acid to produce aluminum sulfate. If they produce 3. 00 g of aluminum sulfate what is their percent yield
The percent yield for the reaction of 1.23 g of aluminum with excess sulfuric acid to produce 3.00 g of aluminum sulfate is 38.46%.
To find the percent yield for the reaction of aluminum with sulfuric acid to produce aluminum sulfate, you need to follow these steps:
1. Write the balanced chemical equation for the reaction:
2 Al + 3 H₂SO₄ → Al₂(SO₄)₃ + 3 H₂
2. Calculate the molar mass of aluminum (Al) and aluminum sulfate (Al₂(SO₄)₃):
Al: 26.98 g/mol
Al₂(SO₄)₃: (2 × 26.98) + (3 × [4 × 16.00 + 32.07]) = 53.96 + 342.15 = 342.15 g/mol
3. Determine the moles of aluminum used in the reaction:
moles of Al = mass of Al / molar mass of Al = 1.23 g / 26.98 g/mol = 0.0456 mol
4. Calculate the theoretical yield of aluminum sulfate based on the moles of aluminum:
moles of Al₂(SO₄)₃ = 0.0456 mol Al × (1 mol Al₂(SO₄)₃ / 2 mol Al) = 0.0228 mol Al₂(SO₄)₃
mass of Al₂(SO₄)₃ = moles of Al₂(SO₄)₃ × molar mass of Al₂(SO₄)₃ = 0.0228 mol × 342.15 g/mol = 7.80 g (theoretical yield)
5. Calculate the percent yield:
percent yield = (actual yield / theoretical yield) × 100% = (3.00 g / 7.80 g) × 100% = 38.46%
So, the percent yield for the reaction of 1.23 g of aluminum with excess sulfuric acid to produce 3.00 g of aluminum sulfate is 38.46%.
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A gas sample having an initial temperature of 80℃ and an initial volume of 135 l is cooled to a final temperature of 12℃ and a final volume of 103 l. if the final pressure of the gas is 1.50 atm, what was the initial pressure?
If the final pressure of the gas is 1.50 atm, the initial pressure would be 2.16 atm.
In order to solve this problem, we need to use the combined gas law equation, which relates the pressure, volume, and temperature of a gas. The combined gas law states that PV/T = constant, where P is pressure, V is volume, and T is temperature.
We know the initial temperature, initial volume, final temperature, final volume, and final pressure of the gas. We can use this information to solve for the initial pressure.
First, we can use the combined gas law to find the constant in the equation:
(Pinitial)(Vinitial)/(Tinitial) = (Pfinal)(Vfinal)/(Tfinal)
Substituting in the values we know, we get:
(Pinitial)(135 L)/(353 K) = (1.50 atm)(103 L)/(285 K)
Solving for Pinitial, we get:
Pinitial = (1.50 atm)(103 L)(353 K)/(285 K)(135 L)
Pinitial = 2.16 atm
Therefore, the initial pressure of the gas was 2.16 atm.
In summary, we used the combined gas law equation to solve for the initial pressure of a gas sample with an initial temperature of 80℃ and an initial volume of 135 l that was cooled to a final temperature of 12℃ and a final volume of 103 l with a final pressure of 1.50 atm. We found that the initial pressure of the gas was 2.16 atm.
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What happens in a decomposition reaction? A. Two ions trade places. B. Two substances combine to form one substance. C. The charges of the atoms change. D. Compounds break down into smaller compounds.
A single compound decomposes into two or more smaller compounds or components during a decomposition reaction. Option D
A number of mechanisms, such as heat, light, or the addition of another molecule, can cause this. A significant quantity of potential energy is often held in the chemical bonds of the reactant component, and this energy is released during the reaction.
For instance, hydrogen peroxide's typical breakdown reaction involves the molecule dissolving into water and oxygen gas:
[tex]2H_2O_2 \rightarrow 2 H_2O + O_2[/tex]
The heat breakdown of calcium carbonate to produce calcium oxide and carbon dioxide gas is another illustration:
[tex]CaO + CO_2 = CaCO_3[/tex]
Decomposition reactions are crucial components of several chemical processes in both nature and industry. They are characterised by the dissolution of bigger molecules into smaller ones. Option D
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The Si unit of hurtz equals one wave passing a fixed point in one _____
The Si unit of Hertz (Hz) represents the frequency of a wave, which is defined as the number of complete cycles of a wave passing a fixed point per second.
In other words, one Hertz equals one wave passing a fixed point in one second. This unit is commonly used to measure the frequency of various types of waves, including sound waves, electromagnetic waves, and radio waves.
For example, if a sound wave has a frequency of 440 Hz, it means that the sound wave completes 440 cycles of compression and rarefaction (the peaks and troughs of the wave) per second. Similarly, if a radio wave has a frequency of 100 MHz (megahertz), it means that the wave completes 100 million cycles per second.
The Hertz unit was named after Heinrich Hertz, a German physicist who was the first to demonstrate the existence of electromagnetic waves. Hertz's experiments in the late 19th century paved the way for the development of modern radio, television, and other forms of wireless communication.
In summary, the Si unit of Hertz equals one wave passing a fixed point in one second, and it is a fundamental unit of measurement for the frequency of various types of waves.
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For a 80- g sample of fused copper catalyst, a volume of 7.6×103 mm3 of nitrogen (measured at standard temperature and pressure, 0 ∘c and 1 atm ) is required to form a monolayer upon condensation. calculate the surface area of the catalyst. (take the area covered by a nitrogen molecule as 0.162 nm2 and recall that, for an ideal gas, pv=nrt , where n is the number of moles of the gas.)
Answer:
First, we need to calculate the number of moles of nitrogen gas required to form a monolayer:
n = (pv) / (rt)
where p is the pressure, v is the volume, r is the ideal gas constant, and t is the temperature in Kelvin.
At standard temperature and pressure, we have:
p = 1 atm
v = 7.6×10^3 mm^3 = 7.6×10^-6 m^3
t = 273 K
r = 8.31 J/(mol K)
So, n = (1 atm x 7.6×10^-6 m^3) / (8.31 J/(mol K) x 273 K) = 3.13×10^-7 mol
Next, we can calculate the number of nitrogen molecules in this amount of gas:
N = n x Na
where Na is Avogadro's number (6.02×10^23 molecules/mol).
N = 3.13×10^-7 mol x 6.02×10^23 molecules/mol = 1.88×10^17 molecules
Finally, we can calculate the surface area of the catalyst covered by these molecules:
A = N x a
where a is the area covered by a nitrogen molecule (0.162 nm^2), converted to m^2.
a = 0.162 nm^2 x (10^-18 m^2/nm^2) = 1.62×10^-20 m^2
A = 1.88×10^17 molecules x 1.62×10^-20 m^2/molecule = 3.05×10^-3 m^2
Therefore, the surface area of the catalyst covered by the nitrogen molecules is approximately 3.05×10^-3 m^2.
How many liters of a 0. 26 M solution of K2(MnO4) would contain 75 g of K2(MnO4)?
1.35 liters of a 0.26 M solution of K2(MnO4) would contain 75 g of K2(MnO4).
To determine the volume of a 0.26 M solution of K2(MnO4) needed to contain 75 g of K2(MnO4), we need to use the formula:
Molarity (M) = moles of solute / volume of solution (L)
First, convert the mass of K2(MnO4) to moles using its molar mass:
Molar mass of K2(MnO4) = 2 * (39.1 g/mol for K) + (54.9 g/mol for Mn) + 4 * (16 g/mol for O) = 214.2 g/mol
Moles of K2(MnO4) = 75 g / 214.2 g/mol ≈ 0.35 moles
Now use the molarity formula to find the volume:
0.26 M = 0.35 moles / volume (L)
Volume (L) = 0.35 moles / 0.26 M ≈ 1.35 L
So, approximately 1.35 liters of a 0.26 M solution of K2(MnO4) would contain 75 g of K2(MnO4).
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If the pressure of a 7. 2 liter sample of gas changes from 735 mmHg to 800 mmHg and the temperature remains constant, what is the new volume of
gas?
06. 62 L
оооо
0 5. 9 L
0 7. 2L
The new volume of gas is 6.62 L when the pressure changes from 735 mmHg to 800 mmHg at a constant temperature.
According to Boyle's Law, at a constant temperature, the pressure and volume of a gas are inversely proportional. This means that as the pressure of the gas increases, its volume decreases, and vice versa. Therefore, we can use this law to find the new volume of gas when the pressure changes from 735 mmHg to 800 mmHg.
Using the formula P1V1 = P2V2, where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume, we can solve for V2.
Plugging in the values given in the question, we get:
735 mmHg x 7.2 L = 800 mmHg x V2
Solving for V2, we get:
V2 = (735 mmHg x 7.2 L) / 800 mmHg
V2 = 6.62 L
Therefore, the new volume of gas is 6.62 L when the pressure changes from 735 mmHg to 800 mmHg at a constant temperature.
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PLEASE HELP
Andrea plans to go fishing in the morning, so she checks the weather forecast. The forecast shows a high-pressure area forming near her fishing spot. Using the weather data below, predict the possible weather conditions for Andrea’s trip.
Time (a.m.) Temperature (°C) Pressure (mb)
7.00 14 995
8.00 14 1001
9.00 14 1113
10.00 15 1120
A.
cloudy skies with minimal precipitation
B.
clear skies with minimal precipitation
C.
cloudy skies with moderate precipitation
D.
clear skies with heavy precipitation
B Answer:
Explanation:
Higher, 1020 mb +, rising pressure and temp are associated with clear skies and low precipitation
A soft lump of clay has water run on top of it. Most of the water and clay runs off the table. After a long while, the water is turned off and allowed to dry. There is no clay left; instead, there are small pebbles and other types of components left on the table.
Which natural process is this modeling?
The natural process being modeled is weathering, specifically physical weathering.
Physical weathering is the process by which rocks and minerals are broken down into smaller pieces without changing their chemical composition. Water is one of the most significant agents of physical weathering.
The scenario described in the question illustrates how water can cause physical weathering by soaking into a lump of clay, then drying out, leaving behind small pebbles and other components. The water expands as it freezes, causing the clay to crack, and as it dries, it evaporates, leaving behind the broken pieces.
Over time, this process can break down larger rocks and minerals into smaller particles, creating sediment that can be transported by wind, water, or ice, and deposited elsewhere. The result of physical weathering is often a mix of angular fragments that have the same composition as the original rock or mineral.
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