Explanation:
Table H lists vapor pressure data for pure water at various temperatures. We can use this data to estimate the vapor pressure of the water in the given system at its final temperature of 80.0°C.
First, we need to calculate the heat absorbed by the water sample during the heating process. We can use the specific heat capacity of water to do this:
q = m * c * ΔT
where q is the heat absorbed, m is the mass of water (100 g), c is the specific heat capacity of water, and ΔT is the temperature change (80°C - 30°C = 50°C).
Plugging in the values, we get:
q = 100 g * 4.18 J/(g*C) * 50 C
q = 20900 J
This tells us that 20,900 joules of energy were absorbed by the water sample during heating.
Next, we need to consider the saturated solution of KCIO3 in the water sample. At 80.0°C, the water is already close to boiling, so it is likely that the vapor pressure of the water in the system is close to the vapor pressure of pure water at this temperature. From Table H, we can see that the vapor pressure of pure water is approximately 356 mmHg at 80.0°C.
Therefore, the vapor pressure of the water in the given system at its final temperature of 80.0°C is approximately 356 mmHg.
The specific heat of gold is 0.129 J/g C. A king gets sold a gold crown but he's unsure if it's pure gold. He takes the crown which weighs 1,130 grams, heats it to 98.8 C, and then places it in 1.34 L of water with a starting point of 25.83 C. The final temperature of the water is 27.84 C. What is the specific heat of the crown and is it pure gold?
We can use the formula:
Q = mcΔT
where Q is the heat absorbed or released, m is the mass, c is the specific heat, and ΔT is the change in temperature.
First, let's calculate the heat absorbed by the crown:
Q1 = mcΔT
Q1 = (1130 g)(0.129 J/g C)(98.8 C - 25.83 C)
Q1 = 107,776.6 J
Next, let's calculate the heat released by the crown into the water:
Q2 = mcΔT
Q2 = (m)(c)(ΔT)
Q2 = (1340 g)(4.184 J/g C)(27.84 C - 25.83 C)
Q2 = 11096.64 J
Since Q1 = -Q2 (heat lost by the crown is equal to heat gained by the water),
mcΔT = -mcΔT
We can then solve for the specific heat of the crown:
c = -(Q2/mΔT)
c = -(11096.64 J)/(1130 g)(27.84 C - 25.83 C)
c = 0.131 J/g C
The specific heat of pure gold is 0.129 J/g C, and the specific heat of the crown is 0.131 J/g C. Since the specific heat of the crown is slightly higher than that of pure gold, it is possible that the crown is not pure gold. However, other factors such as impurities or alloying metals can also affect the specific heat, so further analysis would be necessary to confirm if the crown is pure gold.
A sample of gas is contained in a 245 mL flask at a temperature of 23.5°C. The gas pressure is 37.8 mm Hg. The gas is moved to a new flask, which is then immersed in ice water, and which has a volume of 54 mL. What is the pressure of the gas in the smaller flask at the new temperature?
The pressure of the gas in the smaller flask at the new temperature is approximately 168.5 mm Hg.
To solve this problem, we can use the combined gas law equation, which relates the initial and final states of a gas sample undergoing changes in pressure, volume, and temperature. The equation is:
[tex]P_1V_1/T_1 = P_2V_2/T_2[/tex]
where [tex]P_1[/tex] and [tex]P_2[/tex] are the initial pressure and final pressure, [tex]V_1[/tex] and [tex]V_2[/tex] are the initial and final volumes, and [tex]T_1[/tex] and [tex]T_2[/tex] are the initial and final temperatures in Kelvin.
[tex]V_1[/tex] = 245 mL
[tex]T_1[/tex] = 23.5°C + 273.15 = 296.65 K
[tex]P_1[/tex] = 37.8 mm Hg
[tex]V_2[/tex] = 54 mL
[tex]T_2[/tex] = 0°C (ice water) + 273.15 = 273.15 K
We need to find [tex]P_2[/tex] . Plug the given values into the equation and solve for [tex]P_2[/tex] :
(37.8 mm Hg * 245 mL) / 296.65 K = (P2 * 54 mL) / 273.15 K
Rearrange the equation to isolate [tex]P_2[/tex] :
[tex]P_2[/tex] = (37.8 mm Hg * 245 mL * 273.15 K) / (296.65 K * 54 mL)
[tex]P_2[/tex] ≈ 168.5 mm Hg
So, the pressure of the gas is approximately 168.5 mm Hg in the smaller flask at the new temperature.
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How many grams of KOH are needed to make 185.5 ml with a concentration of 5 M?
Type your answer...
To calculate the mass of KOH needed to make a 5 M solution in 185.5 mL, we need to use the formula:
mass = moles × molar mass
where moles is the amount of KOH in moles and molar mass is the mass of one mole of KOH.
We can calculate the moles of KOH as follows:
moles = Molarity × Volume (in liters)
First, we need to convert the volume from milliliters to liters:
185.5 mL = 0.1855 L
Now we can calculate the moles of KOH:
moles = 5 M × 0.1855 L = 0.9275 moles
The molar mass of KOH is 56.11 g/mol. Therefore, the mass of KOH needed is:
mass = 0.9275 moles × 56.11 g/mol = 52.05 g
Therefore, 52.05 grams of KOH are needed to make a 5 M solution in 185.5 mL.
How many moles are in 28g of CO2?
Answer:
0.636 moles of CO2
Explanation:
The molar mass of CO2 is 44.01 g/mol (12.01 g/mol for one carbon atom and 2 x 16.00 g/mol for two oxygen atoms). To find the number of moles in 28g of CO2, you can divide the mass by the molar mass: 28g / 44.01 g/mol = 0.636 moles of CO2.
6. A 90.0 gram sample of an unknown solid is heated to 80 °C and placed into a calorimeter containing 120 grams of water at 24 °C. If the final temperature of the solid sample and the water is 32 °C, what is the specific heat of solid?
PLEASE SHOW WORK
Answer:
1.02 J/g°C.
Explanation:
We can use the equation:
q = m * c * ΔT
where q is the heat absorbed or released, m is the mass of the substance (in grams), c is the specific heat, and ΔT is the change in temperature (in Celsius).
First, we can calculate the heat gained by the water:
q_water = m_water * c_water * ΔT_water
where m_water is the mass of the water (in grams), c_water is the specific heat of water (4.184 J/g°C), and ΔT_water is the change in temperature of the water.
m_water = 120 g
c_water = 4.184 J/g°C
ΔT_water = (32°C - 24°C) = 8°C
q_water = (120 g) * (4.184 J/g°C) * (8°C) = 4009 J
This means that the heat lost by the unknown solid is equal to the heat gained by the water:
q_solid = -q_water
q_solid = -4009 J
Next, we can calculate the change in temperature of the solid:
ΔT_solid = (32°C - 80°C) = -48°C
Now, we can solve for the specific heat of the solid:
q_solid = m_solid * c_solid * ΔT_solid
-4009 J = (90.0 g) * c_solid * (-48°C)
c_solid = -4009 J / (90.0 g * -48°C)
c_solid = 1.02 J/g°C
Therefore, the specific heat of the unknown solid is 1.02 J/g°C.
which one have least PH
a. CH3CH2COOH
b. CH2CLCH2COOH
c. CH3CHCL2COOH
d. CH3CH2CH2COOH
CH₃CHCl₂COOH is 2,2-dichloropropanoic acid, with the least pH, option (c) is correct.
pH is a measure of the acidity or basicity of a solution. A lower pH indicates a higher acidity. Acidity is due to the presence of hydrogen ions (H⁺) in a solution. The more the concentration of H⁺, the lower the pH. CH₃CH₂COOH is propanoic acid, which has a pH of around 4.9.
CH₂ClCH₂COOH is 2-chloropropanoic acid, which has a pH of around 2.8 due to the electron-withdrawing effect of the chlorine atom. CH₃CH₂CH₂COOH is butanoic acid, which has a pH of around 4.8. Thus, CH₃CHCl₂COOH is 2,2-dichloropropanoic acid, which has the least pH among the given options, around 1.5 due to the presence of two electron-withdrawing chlorine atoms, option (c) is correct.
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draw the lewis structure of ch3br
The Lewis structure of the compound[tex]CH_{3} Br[/tex] is shown in the image attached.
What is the Lewis structure?The Lewis structure of a molecule or ion is produced by arranging the atoms in a manner that lessens the attraction between their valence electron pairs and then distributes the valence electrons among the atoms to form covalent bonds.
The octet rule, which states that atoms normally gain or lose electrons to obtain a stable configuration with eight valence electrons, frequently serves as a guidance when arranging electrons in the Lewis structure.
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If an atom loses an electron, what will its resulting charge be?
Answer:
If an atom loses or gains electrons, it will become a positively or negatively charged particle, called an ion. The loss of one or more electrons results in more protons than electrons and an overall positively charged ion, called a cation.
Hope it helped! :)
Does anyone have Personal Care services on E2020
Here are some questions on Personal Care services on E2020 are:
A client with a new ileostomy has been home for four days. The HHA is giving the client a bath and notices that the pouch is full. The HHA should say to the client: D. "I'll empty the pouch for you."A client is bedridden at home and has an infected draining sacral wound. The infection control supplies that should be kept in the home is: Gloves.What is infection?An infection is the entrance and growth of dangerous microorganisms in the body that harm the host, such as bacteria, viruses, fungus, or parasites.
Infections can be systemic (affecting the entire body) or localized (affecting a particular area of the body), and they can be moderate to severe.
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The change in enthalpy (AH, ) for a reaction is -25.8 kJ mol.
The equilibrium constant for the reaction is 1.4 × 103 at 298 K.
What is the equilibrium constant for the reaction at 655 K?
The equilibrium constant for the reaction at 655 K is [tex]e^{6.96}[/tex] ≈ 1.05 × 10^3.
The equilibrium constant (K) for a reaction is related to the change in Gibbs free energy (ΔG) through the equation:
ΔG = -RTlnK
where R is the gas constant, T is the temperature in kelvin, and ln is the natural logarithm. Since ΔG and ΔH (the change in enthalpy) are related by the equation:
ΔG = ΔH - TΔS
where ΔS is the change in entropy, we can rearrange the first equation to get:
lnK = -ΔH ÷ RT + ΔS ÷ R
At 298 K, we can use the given values of ΔH and K to solve for ΔS:
lnK = -ΔH ÷ RT + ΔS ÷ R
ln(1.4 × 10³) = (-(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 298 K)) + ΔS ÷ 8.314 J/mol K
ΔS = 78.2 J/mol K
Now we can use the equation above to solve for lnK at 655 K, using the same value of ΔH and the newly calculated value of ΔS:
lnK = -ΔH ÷ RT + ΔS ÷ R
lnK = -(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 655 K) + (78.2 J/mol K) ÷ 8.314 J/mol K
lnK = 6.96
e ≈ 1.05 × 10³
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Convert the following number
into correct scientific notation.
0.0602 x 10^25
[ ? ] × 10 [ ? ]
The number is converted to 60. 2 × 10²²
What are index forms?Index forms are simply described as mathematical forms that are used in the representation of numbers that are too small or too large in more convenient forms.
These index forms are also referred to as scientific notation or standard forms.
Some rules of index forms are;
Add the exponents when multiplying forms of the same basesSubtract the exponents when dividing forms of the same basesFrom the information given, we have that;
0. 0602 × 10 ²⁵
Subtract three from the exponent value and move three spaces right, we have;
60. 2 × 10²⁵⁻³
60. 2 × 10²²
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Please help thanks so much!!!!!!!!!!!!
The total mass of products obtained when 130 g of zinc react completely with HCl is 274 g (3rd option)
How do i determine the total mass of products obtained?First, we shall determine the mass of each product obtained. Details below:
For ZnCl₂
2HCl + Zn -> ZnCl₂ + H₂
Molar mass of Zn = 65 g/molMass of Zn from the balanced equation = 1 × 65 = 65 g Molar mass of ZnCl₂ = 135 g/molMass of ZnCl₂ from the balanced equation = 1 × 135 = 135 gFrom the balanced equation above,
65 g of Zn reacted to produce 135 g of ZnCl₂
Therefore,
130 g of Zn will react to produce = (130 × 135) / 65 = 270 g of ZnCl₂
Thus, the mass of ZnCl₂ obtained is 270 g
For H₂
2HCl + Zn -> ZnCl₂ + H₂
Molar mass of Zn = 65 g/molMass of Zn from the balanced equation = 1 × 65 = 65 g Molar mass of H₂ = 2 g/molMass of H₂ from the balanced equation = 1 × 2 = 2 gFrom the balanced equation above,
65 g of Zn reacted to produce 2 g of H₂
Therefore,
130 g of Zn will react to produce = (130 × 2) / 65 = 4 g of H₂
Thus, the mass of H₂ obtained is 4 g
Finally, we shall determine the total mass of the product produced. Details below:
Mass of ZnCl₂ = 270 gMass of H₂ = 4 gTotal mass of product =?Total mass of product = mass of ZnCl₂ + mass of H₂
Total mass of product = 270 + 4
Total mass of product = 274 g (3rd option)
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1. How many joules of heat is needed to heat 68.00 grams of aluminum foil from 55.00 °C to 93.00 °C if aluminum has a specific heat of 0.90 J/g °C?
2. Which of the following equations is an exothermic reaction?
Answer:
7. C. 2326 J
8. B
Explanation:
7. Use the equation q=m*c* change in temp, where m is mass, c is specific heat capacity.
q= 68 g* (0.9 J/g*c) * (93-55) C
q= 2326 J
8. An exothermic reaction is characterized by a negative delta H (change in enthalpy) since energy is released during the reaction. B is the only choice with a negative delta H.
A zinc chloride solution is prepared by dissolving 0.316 g of anhydrous zinc chloride in 100.0 mL of H2O.
What mass of zinc chloride is present in 19.97 mL of that solution.
A zinc chloride solution is prepared by dissolving 0.316 g of anhydrous zinc chloride in 100.0 mL of [tex]H_2O[/tex] . The mass of zinc chloride present in 19.97 mL of the solution is 0.316 g.
We can use the formula:
C1V1 = C2V2
where C1 is the concentration of the original solution, V1 is the volume of the original solution, C2 is the concentration of the final solution, and V2 is the volume of the final solution.
First, let's calculate the concentration of the original solution:
concentration = (0.316 g) / (100.0 mL) = 0.00316 g/mL
Now, we can use the formula to find the mass of zinc chloride in 19.97 mL of the solution:
C1V1 = C2V2
0.00316 g/mL x 100.0 mL = C2 x 19.97 mL
C2 = (0.00316 g/mL x 100.0 mL) / 19.97 mL
C2 = 0.01583 g/mL
So the concentration of zinc chloride in the final solution is 0.01583 g/mL.
Now we can use this concentration to calculate the mass of zinc chloride in 19.97 mL of the solution:
mass = concentration x volume
mass = 0.01583 g/mL x 19.97 mL
mass = 0.316 g
Therefore, there are 0.316 g of zinc chloride present in 19.97 mL of the solution.
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Mark needs to determine how much the temperature of a solution changes during a chemical reaction. Which tool does he need?
Mark would need a thermometer to determine the temperature change of a solution during a chemical reaction. A thermometer is a tool used to measure temperature and can be used to monitor and record changes in temperature during a chemical reaction. So the answer is thermometer .
There are different types of thermometers, such as liquid-in-glass thermometers, bimetallic strip thermometers, digital thermometers, and infrared thermometers, among others. The choice of thermometer depends on the specific requirements of the experiment or process being carried out.
By measuring the initial and final temperatures of the solution before and after the chemical reaction, Mark can determine the temperature change, which is an important parameter in many chemical reactions as it provides information about the heat energy involved in the reaction, and helps in understanding the thermodynamics and kinetics of the process. Therefore the answer is thermometer .
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Please help I appreciate it thanks!!!!!!!!!!!!!!!!!!!!!!
The correct molar mass for nickel chloride is 94.14 g/mol (option C).
How to calculate molar mass?Molar mass is the mass of a given substance divided by its amount, measured in moles. It is commonly expressed in grams (sometimes kilograms) per mole.
The molar mass of a substance can be calculated by summing up the atomic masses of the element components.
According to this question, the atomic mass of nickel is 58.693 amu while that of chlorine gas is 35.45 amu. The molar mass of nickel chloride can be calculated as follows;
molar mass = 35.45 amu + 58.693 amu = 94.14 g/mol
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Pleas help!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
_______________________________
2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)
Moles of NA = Given Mass (g) ÷ Molecular Mass (g/mol)
= 27.5 ÷ 22.9897
= 1.196 mol
Moles of H2 Produced = Mol of NA × 1 mol H2 ÷ 2 Mol NA
= 1.196 × 1 ÷ 2
= 0.60 mol
Number of Molecules = Moles × Avogadro's Number
= 0.60 × 6.023 × 10²³ mol - 1
= 3.61 × 10²³
The Number of Molecules of Hydrogen Gas Produced When Added To Water Is 3.61 × 10²³
_________________________________
WHEN SOME PEOPLE HAVE AN UPSET STOMACH, THEY TAKE A SODA TABLET LIKE
TUMS TO NEUTRALIZE THEIR STOMACH ACID.
THE REACTION IS HYDROCHLORIC ACID PLUS SODIUM BICARBONATE MAKES SALT,
CARBON DIOXIDE (THAT'S WHY SOME PEOPLE BURP) AND WATER.
HOW MUCH CARBON DIOXIDE AND SALT (IN GRAMS) ARE PRODUCED IF A 2 GRAM
TABLET OF SODIUM BICARBONATE IS TAKEN TO REACT WITH 18 GRAMS OF
HYDROCHLORIC ACID?
The balanced chemical equation for the reaction between hydrochloric acid (HCl) and sodium bicarbonate [tex](NaHCO_3)[/tex] is:
[tex]HCl + NaHCO_3\ - > NaCl + CO_2 + H_2O[/tex]
The coefficients in the balanced equation show that 1 mole of HCl reacts with 1 mole of [tex]NaHCO_3[/tex] to produce 1 mole of NaCl, 1 mole of [tex]CO_2[/tex], and 1 mole of [tex]H_2O[/tex]. We need to find the number of moles of [tex](NaHCO_3)[/tex] present in the tablet.
2 grams of [tex]NaHCO_3[/tex] is equivalent to 0.02 moles, and 18 grams of HCl is equivalent to 0.45 moles. Since [tex](NaHCO_3)[/tex] is limiting reagent, only 0.02 moles of NaCl and [tex]CO_2[/tex] will be produced. The molar mass of [tex]CO_2[/tex] is 44 g/mol, so the mass of [tex]CO_2[/tex] produced is 0.88 g. The molar mass of NaCl is 58.44 g/mol, mass of NaCl produced is 1.17 g.
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25 points and I’ll mark as brainliest!!! Tasks are in the picture.
Answer:
5. 0.566 g
6. A. 100 times more
Explanation:
5. The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration. For a solution with pH=2, the concentration of hydrogen ions is 10^-2 mol/L. Since HBr is a strong acid, it dissociates completely in water to produce H+ and Br- ions. Therefore, the concentration of HBr in the solution is also 10^-2 mol/L.
The molar mass of HBr is 80.91194 g/mol
So, in a 700 mL solution (0.7 L), there are
0.7 L * 10^-2 mol/L = 0.007 mol of HBr.
This corresponds to 0.007 mol * 80.91194 g/mol = 0.566 g of HBr dissolved in the solution.
6. The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration. This means that for each decrease in pH by 1 unit, the hydrogen ion concentration increases by a factor of 10. Since the difference in pH between the two solutions is 3 units (6-3=3), the hydrogen ion concentration in the solution with pH=3 is 10^3 = 100 times more than in the solution with pH=6.
How are models used in chemistry? How does evidence change these models?
Answer: As they develop theories, chemists use models to attempt to explain their findings. Chemists assess the model they are using as new evidence becomes available and, if required, continue to refine it by making modifications.
Explanation:
A sample of an ideal gas has a volume of 3.75 L
at 10.60 ∘C
and 1.80 atm.
What is the volume of the gas at 23.20 ∘C
and 0.990 atm?
The volume of the gas at 23.20∘C and 0.990 atm is 7.12L.
How to calculate volume?The volume of a gas can be calculated using the combined gas law equation as follows;
PaVa/Ta = PbVb/Tb
Where;
Pa, Va and Ta = initial pressure, volume and temperature respectively Pb, Vb and Tb = final pressure, volume and temperature respectivelyAccording to this question, a sample of an ideal gas initially has a volume of 3.75 L at 10.60 ∘C and 1.80 atm. The resulting volume can be calculated as follows;
1.8 × 3.75/283.6 = 0.990 × Vb/296.2
0.0238 × 296.2 = 0.990Vb
Vb = 7.0498 ÷ 0.990
Vb = 7.12L
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What is the molar volume of CO2 at 39 C and 652 torr?
The molar volume of a gas can be calculated using the ideal gas law:
PV = nRT
where P is the pressure of the gas in atmospheres (atm), V is the volume of the gas in liters (L), n is the number of moles of gas, R is the ideal gas constant (0.08206 L·atm/mol·K), and T is the temperature of the gas in Kelvin (K).
To solve for the molar volume of CO2 at 39°C (312 K) and 652 torr (0.859 atm), we can rearrange the ideal gas law as follows:
V = (nRT) / P
First, we need to calculate the number of moles of CO2. We can use the following equation, which relates the pressure, volume, number of moles, and temperature of a gas:
PV = nRT
Solving for n, we get:
n = (PV) / (RT)
Substituting the given values, we get:
n = (0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)
Now we can substitute this expression for n into the equation for the molar volume:
V = (nRT) / P
V = [(0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)] * (0.08206 L·atm/mol·K * 312 K) / (0.859 atm)
Simplifying, we get:
V = 24.45 L/mol
Therefore, the molar volume of CO2 at 39°C and 652 torr is 24.45 L/mol.
Given Equation (Balance it) :
C2H4O2 + NaHCO3 —> NaC2H3O2 + H2O + CO2
Word Problem:
If you have 100 mg of Acetic Acid (C2H4O2) and 10 mg of NaHCO3 (Sodium Bicarbonate), how many grams of CO2 can be produced ?
also determine the theoretical yield of the chemical reaction.
C₂H₄O₂ + NaHCO₃ —> NaC₂H₃O₂ + H₂O + CO₂ the amount of Carbon dioxide produced is 5.28 mg.
Is the reaction between acetic acid and sodium bicarbonate exothermic or endothermic?Water, CO₂ , and C₂H₃NaO₂ were produced when acetic acid and NaHCO₃ were combined. The chemistry is as follows: The reaction between vinegar and baking soda was endothermic.
Acetic acid: 2(12.01 g/mol) + 4(1.01 g/mol) + 2(16.00 g/mol)
= 60.05 g/mol
NaHCO₃ 22.99 g/mol + 1.01 g/mol + 3(16.00 g/mol)
= 84.01 g/mol
100 mg of Acetic acid is equal to 0.1 g, and 10 mg of NaHCO₃ is equal to 0.01 g.
Number of moles of Acetic acid = 0.1 g / 60.05 g/mol
= 0.00167 mol
Number of moles of NaHCO₃ = 0.01 g / 84.01 g/mol
= 0.00012 mol
Since NaHCO₃ has fewer moles, it is the limiting reactant.
Therefore, 0.00012 mol of NaHCO₃ will produce 0.00012 mol of CO₂
The mass of CO₂ produced can be calculated as follows:
Mass of CO₂ = Number of moles of CO₂ x Molar mass of CO₂
Mass of CO₂ = 0.00012 mol x 44.01 g/mol
= 0.00528 g or 5.28 mg
Therefore, the amount of CO₂ produced is 5.28 mg.
The theoretical yield of CO₂ is 0.00012 mol x 44.01 g/mol
= 0.00528 g or 5.28 mg.
This is equal to the actual yield of CO₂ produced.
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Which
thermochemical
equation
corresponds to
the graph?
Answer: C
Explanation:
Answer: C
Explanation:
The table below shows the vapor pressure of water at various temperatures.
Temp(degC) Vapor Pressure (mmHg)
17
14.5
18
15.5
19
16.5
20
17.5
21
18.7
22
19.8
During an experiment 675 mL of helium gas is collected over water at 22 degC. The air pressure in the lab is 0.926 atm. What is the partial pressure of the dry helium collected?
The partial pressure of the Helium gas is 0.9 atm.
What is the partial pressure of gas collected over water?The pressure that a gas exerts on its own when it is collected over water, independent of the pressure that the water vapor in the collecting vessel also produces, is known as its partial pressure.
When gas is collected over water, some of the water vapor will dissolve in it and change the overall pressure in the collecting vessel. Water vapor has its own partial pressure, which is affected by the relative humidity and temperature of the air around it. This is why it behaves in this way.
We have that;
Vapor pressure of the gas = 19.8 mmHg or 0.026 atm
Partial pressure of the Helium gas = 0.926 atm - 0.026 atm
= 0.9 atm
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ichiometry in space
A typical space shuttle crew consists of six individuals and
each CCC contains 750 g of LIOH. Assuming that each crew
member expels 42.0 g of CO₂ per hour on average, and that
a mission is scheduled to last 18 days, how many CCCS must
be carried on board the space
shuttle?
- By knowing the recipe (balanced chemical equation), and
some molar masses, I can calculate this answer.
We need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.
What is the amount of CO2 absorbed?To solve this problem, we need to use the following information:
Each crew member expels 42.0 g of CO2 per hour.The mission is scheduled to last 18 days.There are 6 crew members on board.Each CCC contains 750 g of LIOH.First, we need to calculate the total amount of CO2 that will be expelled during the mission:
Total CO2 = 6 crew members x 42.0 g CO2/hour x 24 hours/day x 18 days = 136,080 g CO2
Next, we need to calculate the amount of LIOH needed to absorb this CO2. The balanced chemical equation for the reaction between CO2 and LIOH is:
CO2 + 2 LIOH → Li2CO3 + H2O
The molar mass of CO2 is 44.01 g/mol, and the molar mass of LIOH is 23.95 g/mol.
This means that 2 moles of LIOH are needed to absorb 1 mole of CO2.
So, to absorb 136,080 g of CO2, we need:
136,080 g CO2 x (1 mol CO2/44.01 g) x (2 mol LIOH/1 mol CO2) x (23.95 g LIOH/1 mol) = 139,648 g LIOH
Since each CCC contains 750 g of LIOH, we need:
139,648 g LIOH / 750 g CCC = 186.2 CCCs
Therefore, we need to carry at least 187 CCCs on board the space shuttle to absorb all the CO2 produced by the crew during the 18-day mission.
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What is the pH of a solution that has a H+ concentration of 1.9x10-6?
The pH of the solution is 5.72, which is slightly acidic.
pH is a measure of the acidity or basicity of a solution. It is defined as the negative logarithm of the hydrogen ion concentration (H+) in a solution. The pH scale ranges from 0 to 14, where a pH of 7 is neutral, pH below 7 is acidic, and pH above 7 is basic. The formula to calculate pH is pH = -log[H+], where [H+] represents the concentration of hydrogen ions in moles per liter.
Given the H+ concentration of 1.9x10-6, we can calculate the pH of the solution as follows:
pH = -log(1.9x10-6) = 5.72
It is important to note that pH is an important factor in various chemical and biological processes. It can affect the solubility of certain substances, enzymatic activity, and the growth and survival of living organisms. Maintaining the appropriate pH is crucial for the proper functioning of these processes.
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Water can dissolve many substances because-
-
it has a partial charge on each side of its molecules
it has a linear molecular shape
it has a nonpolar molecular structure
it has the molecular formula H₂O
Answer:
Water can dissolve many substances because it has a partial charge on each side of its molecules.
Explanation:
Water is a polar molecule, meaning that it has an uneven distribution of electrons between its hydrogen and oxygen atoms. This creates a partial negative charge on the oxygen side of the molecule and a partial positive charge on the hydrogen side. These partial charges allow water molecules to attract and surround other charged or polar molecules, such as ions and polar compounds, and separate them from each other. This process of surrounding and separating other substances in a solution is known as hydration or dissolution, and it is what allows water to dissolve many substances. Therefore, the correct option is: "it has a partial charge on each side of its molecules."
How many grams of O are in 615g of N2O?
There are approximately 223.2 grams of oxygen in 615 grams of N2O.
To find the number of grams of O in 615g of N2O, we first need to understand the chemical formula of N2O. N2O is a compound made up of two nitrogen atoms (N) and one oxygen atom (O). Therefore, the molecular weight of N2O would be:
(2 x atomic weight of N) + (1 x atomic weight of O)
= (2 x 14.01 g/mol) + (1 x 16.00 g/mol)
= 44.01 g/mol
Now, to calculate the number of grams of O in 615g of N2O, we need to know the proportion of O in the compound. Since there is only one oxygen atom in each molecule of N2O, we can find the proportion of O by dividing the atomic weight of O by the molecular weight of N2O:
Atomic weight of O / Molecular weight of N2O
= 16.00 g/mol / 44.01 g/mol
= 0.363
This means that oxygen makes up 36.3% of the total weight of N2O. To find the number of grams of O in 615g of N2O, we can multiply the total weight by the proportion of O:
615g x 0.363
= 223.2g
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Here are some data from a similar experiment, to determine the empirical formula of on oxide of tin.
Calculate the empirical formula according to these data.
Mass of crucible, cover, and tin sample 21.76 g
Mass of empty crucible with cover 19.66 g
Mass of crucible and cover and sample,
after prolonged heating gives constant weight 22.29 g
The information given can be used to construct the empirical formula for a tin oxide. We must first determine the mass of tin in the sample. This may be achieved by deducting the mass of the crucible, cover, and sample (21.76 g) from the mass of the empty crucible and cover (19.66 g).
This gives us a mass of 2.10 g of tin in the sample. The mass of oxygen in the sample must then be determined. To achieve this, we must deduct the mass of the crucible, cover, and sample (21.76 g) from the mass of the same components (22.29 g) prior to protracted heating. This provides us with an oxygen mass of 0.53 g.
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