Question 1

Which impurity in mined coal, when burned, contributes to the production of acid rain?

Accepted Answer

When coal is burned, sulfur dioxide is released into the atmosphere. This sulfur dioxide can react with water and other chemicals in the atmosphere to form sulfuric acid, which contributes to acid rain. Therefore, the impurity in mined coal that contributes to the production of acid rain is sulfur.

Question 2

Calculate the mean free path in a sample of oxygen gas (M = 3.20 × 10^-2 kg/mol) at 35°C and 1.7 atm. Assume that the diameter of an O₂ molecule is 300 pm.

Accepted Answer

The mean free path is given by the equation:$$\lambda = \frac{k_BT}{4\pi r^2 P N_A}$$where:* $k_B$ is the Boltzmann constant ($1.38 	imes 10^{-23}$ J/K)* $T$ is the temperature in Kelvin (35°C = 308 K)* $r$ is the radius of the molecule ($300$ pm = $3 	imes 10^{-10}$ m)* $P$ is the pressure in Pascals (1.7 atm = $1.7 	imes 101325$ Pa)* $N_A$ is the Avogadro constant ($6.022 	imes 10^{23}$ mol$^{-1}$)Substituting these values into the equation, we get:$$\lambda = \frac{(1.38 	imes 10^{-23} 	ext{ J/K})(308 	ext{ K})}{4\pi (3 	imes 10^{-10} 	ext{ m})^2 (1.7 	imes 101325 	ext{ Pa})(6.022 	imes 10^{23} 	ext{ mol}^{-1})}$$$$\lambda = 6.0 	imes 10^{-7} 	ext{ m}$$Therefore, the mean free path is $6.0 	imes 10^{-7}$ m, which is closest to choice A, $0.6 	imes 10^{-7}$ m.

Question 3

The number of wall impacts per second versus the square root of Kelvin temperature for 1 mol of an ideal gas at constant volume
Which graph represents the plot?

Accepted Answer

The number of wall impacts per second is proportional to the square root of temperature for an ideal gas at constant volume. This relationship is given by the Maxwell-Boltzmann distribution. The graph in choice C shows a linear relationship between the square root of temperature and the number of wall impacts per second, which is consistent with the Maxwell-Boltzmann distribution. The other graphs do not show a clear linear relationship between these variables.

Question 4

A gaseous binary compound (which is known to contain nitrogen) has a density 1.94 times that of oxygen gas (at the same temperature and pressure). When 1.31 g of the compound is completely burned in excess oxygen, 1.21 g of water is formed. Determine the formula of the compound.

Accepted Answer

The answer of A gaseous binary compound (which is known...

Question 5

Gas A (MM = 36.0 g/mol) and gas B (MM = 62 g/mol) are present in a mixture that contains 50 molecules A : 326 molecules B. If these gases effuse through a pinhole into a neighboring evacuated chamber, what will be the ratio of A:B in the chamber?

Accepted Answer

The answer of Gas A (MM = 36.0 g/mol) and...

Question 6

Consider the ideal pressure equation for gases, where a is the proportionality constant, n is the moles of molecules, and V is the gas volume. Identify the correct statement(s) about the proportionality constant. 1. A low value for a reflects weak intermolecular forces among the gas molecules. 2. A high value for a reflects weak intermolecular forces among the gas molecules. 3. Among the gases H₂, N₂, CH₄, and CO₂, H₂ has the lowest value for a.

Accepted Answer

The ideal gas equation is PV=nRT, and the proportionality constant in this equation is R. The equation given in the question does not specify which constant is being referred to as "a." Option 1 is incorrect because weak intermolecular forces result in gases occupying more space, and hence a greater value of V. Option 2 is incorrect because a high value of the proportionality constant would indicate a greater effect of pressure on the gas, which is not related to intermolecular forces. Option 3 is correct because H₂ has the strongest intermolecular forces among the given gases, resulting in a lower value of "a" in the ideal gas equation.

Question 7

A sample of helium gas has been contaminated with argon gas. At 1 atm and 25°C, the density of the mixture is 0.200 g/L. What is the volume percent argon in the sample?

Accepted Answer

The answer of A sample of helium gas has been...

Question 8

Near sea level, the atmosphere is composed of 78% nitrogen and 20% oxygen. Other trace gases make up the remaining 2%. At room temperature,

Accepted Answer

At a given temperature, lighter gas molecules (like nitrogen) move faster on average than heavier ones (like oxygen). However, due to the distribution of molecular speeds, some nitrogen molecules can move slower than some oxygen molecules, and vice versa.

Question 9

A certain element (Z) reacts to form three gaseous compounds. Consider the following data (pressure = 1.0 atm).  
Determine the identity of element Z.

Accepted Answer

The answer of A certain element (Z) reacts to form...

Question 10

Determine the collision frequency for an oxygen molecule (M = 3.20 × 10^-2 kg/mol) in a sample of pure oxygen gas at 35°C and 1.7 atm. Assume that the diameter of an O₂ molecule is 300 pm.

Accepted Answer

The collision frequency can be calculated using the formula: $ Z = \sqrt{2} \pi d^2 n \bar{v} $, where $ d $ is the diameter of the molecule, $ n $ is the number density, and $ \bar{v} $ is the average speed of the molecules. Using the given values and converting units appropriately, the collision frequency is approximately $ 7 \times 10^9 $ s$^{-1}$.

Question 11

NOTES:general chemistry
-A scrubber removes the sulfur dioxide from the exhaust gas before it is emitted from a power plant stack. Which of the following compounds is used in the scrubbing process?

Accepted Answer

Powdered limestone, also known as calcium carbonate, is commonly used in the scrubbing process to react with sulfur dioxide and produce calcium sulfite, which can then be oxidized to form gypsum.

Question 12

With respect to the Maxwell-Boltzmann probability distribution function of molecular speeds, which of the following is true?

Accepted Answer

The answer of With respect to the Maxwell-Boltzmann probability distribution...

Question 13

A gaseous mixture is 50% helium gas and 50% nitrogen gas by mass. Determine the percent of the force on the container walls arising from the helium and the ratio of the number of helium impacts to the number of nitrogen impacts on the walls of the vessel.

Accepted Answer

The answer of A gaseous mixture is 50% helium gas...

Question 14

Force per impact versus the molar mass of the ideal gas
Which graph represents the plot?

Accepted Answer

The answer of Force per impact versus the molar mass...

Question 15

Suppose a sealed flask contains 1.0 L of oxygen gas that is completely converted to ozone (O₃) at the same temperature. Calculate the ratio of the new pressure to the original pressure and the ratio of the number of impacts of ozone molecules with the walls of the container to the number of impacts of oxygen molecules with the walls of the container.

Accepted Answer

The answer of Suppose a sealed flask contains 1.0 L...

Question 16

​Complete the following conversion:
1 atm = 760 mm Hg = _____ torr = _____ pascals
​

Accepted Answer

- 1 atm = 760 mm Hg (given)
- 1 torr = 1 mm Hg (definition of torr)
- Therefore, 1 atm = 760 torr
- 1 pascal (Pa) = 1 N/m^2 (definition of pascal)
- 1 atm = 101,325 Pa (standard atmospheric pressure)
- Therefore, 1 atm = 101,325/760 torr ≈ 133.32 torr
- Thus, the answer is A: 760 mm Hg = 760 torr = 133.32 kPa.

Question 17

Consider the decomposition of C₅H₆O₃ as follows: When a 5.63-g sample of pure C₅H₆O₃ was sealed into an otherwise empty 2.50-L flask and heated to 200°C, the pressure gradually rose to 1.63 atm and remained at that value. Calculate the fraction of C₅H₆O₃ (by moles) that decomposed.

Accepted Answer

The answer of Consider the decomposition of C₅H₆O₃ as follows:...

Question 18

Based on the van der Waals equation of state  Which of the following molecules - hydrogen chloride, nitrogen dioxide, or sulfur dioxide - should behave most like an ideal gas.

Accepted Answer

The van der Waals equation of state takes into account the intermolecular forces present in a gas, which makes it more accurate than the ideal gas law. However, the closer a molecule is to an ideal gas, the less its intermolecular forces will affect its behavior. Hydrogen chloride (HCl) is a polar molecule with strong intermolecular forces due to its dipole-dipole interactions, making it the least ideal gas-like molecule of the options given. Nitrogen dioxide (NO2) and sulfur dioxide (SO2) are also polar with dipole-dipole interactions, but they have larger molecular sizes compared to HCl, causing more significant deviations from ideal gas behavior. Out of the given options, sulfur dioxide is expected to have the least deviation from ideal gas behavior due to its slightly larger molecular size compared to nitrogen dioxide. However, since the van der Waals equation of state requires knowledge of both pressure and volume, option B is not a valid choice.

Quiz 5: Gases

Which impurity in mined coal, when burned, contributes to the production of acid rain?

Calculate the mean free path in a sample of oxygen gas (M = 3.20 × 10^-2 kg/mol) at 35°C and 1.7 atm. Assume that the diameter of an O₂ molecule is 300 pm.

The number of wall impacts per second versus the square root of Kelvin temperature for 1 mol of an ideal gas at constant volume Which graph represents the plot?

A gaseous binary compound (which is known to contain nitrogen) has a density 1.94 times that of oxygen gas (at the same temperature and pressure). When 1.31 g of the compound is completely burned in excess oxygen, 1.21 g of water is formed. Determine the formula of the compound.

Gas A (MM = 36.0 g/mol) and gas B (MM = 62 g/mol) are present in a mixture that contains 50 molecules A : 326 molecules B. If these gases effuse through a pinhole into a neighboring evacuated chamber, what will be the ratio of A:B in the chamber?

A sample of helium gas has been contaminated with argon gas. At 1 atm and 25°C, the density of the mixture is 0.200 g/L. What is the volume percent argon in the sample?

Near sea level, the atmosphere is composed of 78% nitrogen and 20% oxygen. Other trace gases make up the remaining 2%. At room temperature,

A certain element (Z) reacts to form three gaseous compounds. Consider the following data (pressure = 1.0 atm). Determine the identity of element Z.

Determine the collision frequency for an oxygen molecule (M = 3.20 × 10^-2 kg/mol) in a sample of pure oxygen gas at 35°C and 1.7 atm. Assume that the diameter of an O₂ molecule is 300 pm.

NOTES:general chemistry -A scrubber removes the sulfur dioxide from the exhaust gas before it is emitted from a power plant stack. Which of the following compounds is used in the scrubbing process?

With respect to the Maxwell-Boltzmann probability distribution function of molecular speeds, which of the following is true?

A gaseous mixture is 50% helium gas and 50% nitrogen gas by mass. Determine the percent of the force on the container walls arising from the helium and the ratio of the number of helium impacts to the number of nitrogen impacts on the walls of the vessel.

Force per impact versus the molar mass of the ideal gas Which graph represents the plot?

Complete the following conversion: 1 atm = 760 mm Hg = _ torr = _ pascals

Based on the van der Waals equation of state Which of the following molecules - hydrogen chloride, nitrogen dioxide, or sulfur dioxide - should behave most like an ideal gas.

Quiz 5: Gases

Which impurity in mined coal, when burned, contributes to the production of acid rain?

Calculate the mean free path in a sample of oxygen gas (M = 3.20 × 10-2 kg/mol) at 35°C and 1.7 atm. Assume that the diameter of an O2 molecule is 300 pm.

The number of wall impacts per second versus the square root of Kelvin temperature for 1 mol of an ideal gas at constant volume Which graph represents the plot?

A gaseous binary compound (which is known to contain nitrogen) has a density 1.94 times that of oxygen gas (at the same temperature and pressure). When 1.31 g of the compound is completely burned in excess oxygen, 1.21 g of water is formed. Determine the formula of the compound.

Gas A (MM = 36.0 g/mol) and gas B (MM = 62 g/mol) are present in a mixture that contains 50 molecules A : 326 molecules B. If these gases effuse through a pinhole into a neighboring evacuated chamber, what will be the ratio of A:B in the chamber?

A sample of helium gas has been contaminated with argon gas. At 1 atm and 25°C, the density of the mixture is 0.200 g/L. What is the volume percent argon in the sample?

Near sea level, the atmosphere is composed of 78% nitrogen and 20% oxygen. Other trace gases make up the remaining 2%. At room temperature,

A certain element (Z) reacts to form three gaseous compounds. Consider the following data (pressure = 1.0 atm). Determine the identity of element Z.

Determine the collision frequency for an oxygen molecule (M = 3.20 × 10-2 kg/mol) in a sample of pure oxygen gas at 35°C and 1.7 atm. Assume that the diameter of an O2 molecule is 300 pm.

NOTES:general chemistry -A scrubber removes the sulfur dioxide from the exhaust gas before it is emitted from a power plant stack. Which of the following compounds is used in the scrubbing process?

With respect to the Maxwell-Boltzmann probability distribution function of molecular speeds, which of the following is true?

A gaseous mixture is 50% helium gas and 50% nitrogen gas by mass. Determine the percent of the force on the container walls arising from the helium and the ratio of the number of helium impacts to the number of nitrogen impacts on the walls of the vessel.

Force per impact versus the molar mass of the ideal gas Which graph represents the plot?

​Complete the following conversion: 1 atm = 760 mm Hg = _____ torr = _____ pascals ​

Consider the decomposition of C5H6O3 as follows: When a 5.63-g sample of pure C5H6O3 was sealed into an otherwise empty 2.50-L flask and heated to 200°C, the pressure gradually rose to 1.63 atm and remained at that value. Calculate the fraction of C5H6O3 (by moles) that decomposed.

Based on the van der Waals equation of state Which of the following molecules - hydrogen chloride, nitrogen dioxide, or sulfur dioxide - should behave most like an ideal gas.

Calculate the mean free path in a sample of oxygen gas (M = 3.20 × 10^-2 kg/mol) at 35°C and 1.7 atm. Assume that the diameter of an O₂ molecule is 300 pm.

Determine the collision frequency for an oxygen molecule (M = 3.20 × 10^-2 kg/mol) in a sample of pure oxygen gas at 35°C and 1.7 atm. Assume that the diameter of an O₂ molecule is 300 pm.

Complete the following conversion: 1 atm = 760 mm Hg = _ torr = _ pascals