A chemistry teacher has 6 liters of a
sodium nitrate solution. She has 24
students in her class and she wants
to divide the solution evenly among
them. How many milliliters of sodium
nitrate solution will each student
receive?

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.

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Here are some questions on Personal Care services on E2020 are:

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 minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3}[/tex] M solution of [tex]Ca(NO_3)_2[/tex] is [tex]6.09 * 10^{-5}[/tex] M.

The solubility product expression for [tex]CaF_2[/tex] is:

[tex]Ksp = [Ca_2^+}][F^-]^2[/tex]

We can use this expression to find the minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3} M[/tex] solution of [tex]Ca(NO_3)_2[/tex].

First, we need to determine the initial concentration of [tex]Ca_2^+[/tex] ions in solution. Since [tex]Ca(NO_3)_2[/tex] dissociates into two [tex]Ca_2^+[/tex] ions and two [tex]NO_3^-[/tex]ions, the initial concentration of [tex]Ca_2^+[/tex] ions is:

[tex]Ca_2^+[/tex] = [tex]2 * 5.25 * 10^{-3} M = 1.05 * 10^{-2} M[/tex]

Next, we can use the solubility product expression to solve for the minimum concentration of fluoride ions required to precipitate [tex]CaF_2[/tex]:

Ksp = [[tex]Ca_2^+[/tex]][tex][F^-]^2[/tex]

[tex]3.9 * 10^{-11} = (1.05 * 10^{-2} M)([F^-]^2)[/tex]

[tex][F^-]^2 = (3.9 * 10^{-11})/(1.05 * 10^{-2} M) = 3.71 * 10^{-9}[/tex]

[tex][F^-] = \sqrt{(3.71 * 10^{-9}) } = 6.09 * 10^{-5} M[/tex]

Therefore, the minimum concentration of fluoride ions necessary to precipitate [tex]CaF_2[/tex] from a [tex]5.25 * 10^{-3}[/tex] M solution of [tex]Ca(NO_3)_2[/tex] is [tex]6.09 * 10^{-5}[/tex]M.

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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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The number is converted to 60. 2 × 10²²

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;

From 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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(a) The formal charge of Cl in the hypochlorite ion (ClO-) is +1.

(b) The formal charge of Cl in the perchlorate ion (ClO4-) with single bonds is +3.

For chlorine (Cl):

Valence electrons: 7

Non-bonding electrons: 6 (3 lone pairs)

Bonding electrons: 2 (1 single bond with oxygen)

Formal charge of Cl = 7 - 6 - (1/2 * 2) = 7 - 6 - 1 = +1

Hence, the formal charge of Cl in the hypochlorite ion is +1.

(c) The oxidation number of Cl in the hypochlorite ion is +1.

(d) The oxidation number of Cl in the perchlorate ion with single bonds is +7.

(e) In a redox reaction, the hypochlorite ion (ClO-) would be more easily reduced because it has a lower oxidation number (+1) compared to the perchlorate ion (+7).

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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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C₂H₄O₂ + NaHCO₃ —> NaC₂H₃O₂ + H₂O + CO₂ the amount of Carbon dioxide produced is 5.28 mg.

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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The aluminum block absorbed 0.875 kJ of heat energy when it was dropped into the coffee.

let's calculate the heat lost by the coffee when it is cooled from its initial temperature of 90.0°C to its final temperature of 55.0°C:

Q1 = m1 * C1 * (90.0°C - 55.0°C)

Q1 = 850 g * 4.184 J/g °C * (90.0°C - 55.0°C)

Q1 = 125660 J

where m1 is the mass of the coffee, C1 is the specific heat of water.

Next, let's calculate the heat gained by the aluminum block when it is heated from 4.4°C to the final temperature of the mixture, which is 55.0°C:

Q2 = m2 * C2 * (55.0°C - 4.4°C)

Q2 = 18 g * 0.89 J/g °C * (55.0°C - 4.4°C)

Q2 = 875.16 J

where m2 is the mass of the aluminum block, and C2 is the specific heat of aluminum.

Since the energy lost by the coffee is gained by the aluminum block, we can set Q1 equal to Q2:

Q1 = Q2

125660 J = 875.16 J + m2 * C2 * (55.0°C - 4.4°C)

Solving for m2, we get:

m2 = (125660 J - 875.16 J) / (0.89 J/g °C * (55.0°C - 4.4°C))

m2 = 152.2 g

Therefore, the mass of the aluminum block that was dropped into the coffee is 152.2 g. To calculate the heat energy absorbed by the aluminum block, we can use the heat gained by the aluminum block that we calculated earlier:

Q2 = 875.16 J

Converting this to kJ, we get:

Q2 = 0.875 kJ

Therefore, the aluminum block absorbed 0.875 kJ of heat energy when it was dropped into the coffee.

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The correct molar mass for nickel chloride is 94.14 g/mol (option C).

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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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.

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.

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.

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.

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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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."

Answer:

39.7

Explanation:

Therefore, the final temperature of the water is 39.7°C.

The total mass of products obtained when 130 g of zinc react completely with HCl is 274 g (3rd option)

First, we shall determine the mass of each product obtained. Details below:

For ZnCl₂

2HCl + Zn -> ZnCl₂ + H₂

From 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

From 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:

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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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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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.

To solve this problem, we need to use the following information:

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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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:

The volume of the gas at 23.20∘C and 0.990 atm is 7.12L.

The volume of a gas can be calculated using the combined gas law equation as follows;

PaVa/Ta = PbVb/Tb

Where;

According 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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Answer: C

Explanation:

Answer: C

Explanation:

Hydrazine, reacts with the oxygen to form the nitrogen gas and the water. The percent yield of the reaction is 3.18 %.

The balanced reaction is :

N₂H₄  + O₂  --->  N₂ + 2H₂O

The mass of the N₂H₄  = 3.55 g

The moles of N₂H₄ = mass / molar mass

The moles of N₂H₄ = 3.55 / 32

The moles of N₂H₄ = 0.110 mol

The theoretical yield = 0.110 mol × 28 g/mol

The theoretical yield = 3.08 g

The gas equation is :

P V = n R T

n = P V / R T

n = (1 × 0.850 ) / ( 0.0823 ×295 )

n = 0.0035 mol

The actual yield = 0.0035 × 28

The actual yield = 0.098 g

The percent yield = ( 0.098 / 3.08 ) × 100 %

The percent yield = 3.18 %.

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The partial pressure of the Helium gas is  0.9 atm.

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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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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the balanced equation and there reactions are as follow:

K₂O + H₂O → 2KOH

The reaction between potassium oxide and water produces potassium hydroxide (KOH).

F₂ + 2NaBr → 2NaF + Br₂

The reaction between fluorine gas and sodium bromide produces sodium fluoride and bromine.

2Ba(CIO3)₂ → 2BaCl₂ + 3O₂

The decomposition of barium chlorate produces barium chloride and oxygen gas.

SrBr₂ + (NH₄)₂CO₃ → SrCO₃ + 2NH₄Br

The reaction between strontium bromide and ammonium carbonate produces strontium carbonate and ammonium bromide.

C₈H₁₈ + 12O₂ → 8CO₂ + 9H₂O

The combustion of octane with oxygen produces carbon dioxide and water.

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