Question 1

You have 41.6 g of O₂ gas in a container with twice the volume as one with CO₂ gas.The pressure and temperature of both containers are the same.Calculate the mass of carbon dioxide gas you have in the container. A)57.2 g B)0.650 g C)28.6 g D)2.60 g E)none of these

Accepted Answer

Since the pressure, temperature, and volume are the same for both containers, we can use the ideal gas law to compare the number of moles of the two gases. PV = nRT Since the pressure, volume, and temperature are the same for both containers, we have: n1 = (PV)/(RT) for O₂ gas in container 1 n2 = 2*(PV)/(RT) for CO₂ gas in container 2 Since the mass of each gas is directly proportional to the number of moles, we can compare the masses of the two gases using the ratio of their number of moles: mass1/mass2 = (n1*MM1)/(n2*MM2) where MM1 and MM2 are the molar masses of O₂ and CO2, respectively. Since MM1 = 44.01 g/mol and MM2 = 28.01 g/mol, we can rearrange the equation to solve for the mass of CO2: mass2 = (n2*MM2*mass1)/(n1*MM1) = (2*28.01*41.6)/(44.01) = 28.6 g. Therefore, the mass of carbon dioxide gas in the container is 28.6 g.

Question 2

A glass column is filled with mercury and inverted in a pool of mercury.The mercury column stabilizes at a height of 729 mm above the pool of mercury.What is the pressure of the atmosphere?
A)1.04 atm
B)0.729 atm
C)0.959 atm
D)456 atm
E)0.639 atm

Accepted Answer

The height of the mercury column (h) is directly proportional to the atmospheric pressure (P). Using the equation P = hρg, where ρ is the density of mercury and g is the acceleration due to gravity, we can calculate the atmospheric pressure.

P = 729 mm Hg x 13.6 g/cm3 x 9.81 m/s2 / 1000 mm/m
P = 0.959 atm (rounded to three significant figures)

Therefore, the pressure of the atmosphere is 0.959 atm, which corresponds to choice C.

Question 3

You have a certain mass of helium gas (He)in a rigid steel container.You add the same mass of neon gas (Ne)to this container.Which of the following best describes what happens? Assume the temperature is constant.
A)The pressure in the container doubles.
B)The pressure in the container increases but does not double.
C)The pressure in the container more than doubles.
D)The volume of the container doubles.
E)The volume of the container more than doubles.

Accepted Answer

The pressure in the container increases but does not double because both helium and neon are noble gases and follow the ideal gas law, which states that pressure is directly proportional to the number of molecules and their average kinetic energy. Since both gases have the same mass, they have the same number of molecules, so the total number of molecules in the container remains constant. Therefore, the pressure increase is due to the fact that the container now has two gases instead of one. However, the pressure increase will not be double because the individual molecules of helium and neon have different masses and therefore different average kinetic energies, resulting in slightly different pressures.

Question 4

Gases generally have
A)low density
B)high density
C)closely packed particles
D)no increase in volume when temperature is increased
E)no decrease in volume when pressure is increased

Accepted Answer

Gases generally have low density because the particles are far apart and have a lot of space between them.

Question 5

Consider a sample of helium gas in a container fitted with a piston,as pictured below.The piston is frictionless,but has a mass of 10.0 kg.How many of the following processes will cause the piston to move away from the base and decrease the pressure of the gas? Assume ideal behavior. 
10.0 kg
$\downarrow$

base $\uarr$
I.heating the helium
II.removing some of the helium from the container
III.turning the container on its side
IV.decreasing the pressure outside the container
A)0
B)1
C)2
D)3
E)4

Accepted Answer

The answer of Consider a sample of helium gas in...

Question 6

Charles's law states that:
A)Equal amounts of gases occupy the same volume at constant temperature and pressure.
B)The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.
C)The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.
D)The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
E)The rates of effusion of gases are inversely proportional to the square roots of their molar masses.

Accepted Answer

Charles's law states that the volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure. This means that as the temperature of a gas increases, its volume will increase proportionally. This relationship can be expressed mathematically as V/T = k, where V is the volume, T is the temperature in Kelvin, and k is a constant.

Question 7

You are holding two balloons,an orange balloon and a blue balloon.The orange balloon is filled with neon (Ne)gas and the blue balloon is filled with argon (Ar)gas.The orange balloon has twice the volume of the blue balloon.Which of the following best represents the mass ratio of Ne:Ar in the balloons?
A)1:1
B)1:2
C)2:1
D)1:3
E)3:1

Accepted Answer

Given that the orange balloon has twice the volume of the blue balloon and both balloons are filled with noble gases (Neon and Argon), the mass ratio depends on the molar mass of the gases and the volume they occupy. Neon has a molar mass of approximately 20 g/mol, and Argon has a molar mass of approximately 40 g/mol. Since the volume of Neon is twice that of Argon but its molar mass is half, the mass of Neon in the orange balloon will be equal to the mass of Argon in the blue balloon, making the mass ratio 1:1.

Question 8

The local weather forecaster reports that the current barometric pressure is 30.4 inches of mercury.What is the current pressure in atmospheres?
A)1.02 atm
B)10.29 atm
C)1.00 atm
D)4.05 atm
E)910 atm

Accepted Answer

The standard atmospheric pressure is defined as being exactly equal to 760 mmHg (millimeters of mercury). To convert inches of mercury to atmospheres, you first convert inches to millimeters (1 inch = 25.4 mm), so 30.4 inches of mercury is 30.4 * 25.4 mmHg = 772.16 mmHg. Since 760 mmHg is equal to 1 atm, 772.16 mmHg is slightly more than 1 atm. The closest answer to this calculation is 1.02 atm.

Question 9

A gas sample is held at constant pressure.The gas occupies 3.62 L of volume when the temperature is 21.6°C.Determine the temperature at which the volume of the gas is 3.42 L.
A)312 K
B)278 K
C)20.4 K
D)295 K
E)552 K

Accepted Answer

The answer of A gas sample is held at constant...

Question 10

Boyle's law states that:
A)Equal amounts of gases occupy the same volume at constant temperature and pressure.
B)The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.
C)The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.
D)The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
E)The rates of effusion of gases are inversely proportional to the square roots of their molar masses.

Accepted Answer

Boyle's law states that for a fixed amount of gas at constant temperature, the volume of the gas is inversely proportional to its pressure. Mathematically, this can be expressed as PV = k, where P is the pressure of the gas, V is the volume of the gas, and k is a constant. Therefore, as the pressure of the gas increases, its volume decreases, and vice versa.

Question 11

Consider a sample of gas in a container on a comfortable spring day.The Celsius temperature suddenly doubles,and you transfer the gas to a container with twice the volume of the first container.If the original pressure was 12 atm,what is a good estimate for the new pressure?
A)3 atm
B)5.5 atm
C)6.4 atm
D)12 atm
E)15 atm

Accepted Answer

Doubling the Celsius temperature approximately doubles the Kelvin temperature, and doubling the volume halves the pressure. Therefore, the new pressure is about $12 atm \times \frac{1}{2} = 6 atm$, making 6.4 atm (C) the closest estimate.

Question 12

Which of the following would represent the greatest pressure?
A)0.680 atm
B)517 mmHg
C)11.4 psi
D)62106 Pa
E)14.1 in Hg

Accepted Answer

The answer of Which of the following would represent the...

Question 13

A physics experiment is conducted at a pressure of 14.4 kPa.What is this pressure in mmHg?
A)18.9 mmHg
B)1.92 mmHg
C)  mmHg
D)108 mmHg
E)  mmHg

Accepted Answer

The answer of A physics experiment is conducted at a...

Question 14

Pressure is
A)defined as the mass that an object exerts when at rest
B)measured in Newtons
C)defined as the number of moles of substance divided by the mass of the substance
D)defined as the force per unit area
E)measured in grams

Accepted Answer

Pressure is defined as the force per unit area. It is commonly measured in units of Newtons per square meter (N/m²) or Pascal (Pa).

Question 15

A balloon has a volume of 2.32 liters at 24.0°C.The balloon is heated to 48.0°C.Calculate the new volume of the balloon.
A)2.32 L
B)2.51 L
C)2.15 L
D)4.64 L
E)1.16 L

Accepted Answer

To find the new volume of the balloon when it is heated, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature in Kelvin, assuming the pressure and the amount of gas remain constant. The formula for Charles's Law is V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature in Kelvin, V2 is the final volume, and T2 is the final temperature in Kelvin.First, convert the temperatures from Celsius to Kelvin by adding 273.15:T1 = 24.0°C + 273.15 = 297.15 KT2 = 48.0°C + 273.15 = 321.15 KNext, solve for V2 using the formula:V2 = V1 * (T2/T1) = 2.32 L * (321.15 K / 297.15 K) ≈ 2.51 L

Question 16

Gaseous chlorine is held in two separate containers at identical temperature and pressure.The volume of container 1 is 1.30 L,and it contains 6.70 mol of the gas.The volume of container 2 is 2.33 L.How many moles of the gas are in container 2?
A)12.0 mol
B)20.3 mol
C)0.452 mol
D)3.74 mol
E)none of these

Accepted Answer

The answer of Gaseous chlorine is held in two separate...

Question 17

The SI unit of pressure is the
A)ampere
B)kilojoule
C)newton
D)gram
E)pascal

Accepted Answer

The SI unit of pressure is pascal (Pa), which is defined as one newton per square meter (N/m²).

Question 18

The air pressure in the inner tube of a tire on a typical racing bike is held at a pressure of about 112 psi.Convert this pressure to atm.
A)0.147 atm
B)7.62 atm
C)0.112 atm
D)0.131 atm
E)112 atm

Accepted Answer

To convert psi to atm, you can use the conversion factor 1 atm = 14.696 psi. So, 112 psi * (1 atm / 14.696 psi) = 7.62 atm.

Question 19

Avogadro's law states that:
A)Equal amounts of gases occupy the same volume at constant temperature and pressure.
B)The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.
C)The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.
D)The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
E)The rates of effusion of gases are inversely proportional to the square roots of their molar masses.

Accepted Answer

Avogadro's law states that equal volumes of gases at the same temperature and pressure contain the same number of particles or molecules. Therefore, equal amounts of gases occupy the same volume at constant temperature and pressure.

Question 20

Body temperature is about 309 K.On a cold day,what volume of air at 276 K must a person with a lung capacity of 2.2 L breathe in to fill the lungs?
A)2.46 L
B)1.97 L
C)2.08 L
D)3.93 L
E)none of these

Accepted Answer

The answer of Body temperature is about 309 K.On a...

Quiz 5: Gases

You have 41.6 g of O₂ gas in a container with twice the volume as one with CO₂ gas.The pressure and temperature of both containers are the same.Calculate the mass of carbon dioxide gas you have in the container.

A glass column is filled with mercury and inverted in a pool of mercury.The mercury column stabilizes at a height of 729 mm above the pool of mercury.What is the pressure of the atmosphere?

You have a certain mass of helium gas (He) in a rigid steel container.You add the same mass of neon gas (Ne) to this container.Which of the following best describes what happens? Assume the temperature is constant.

Gases generally have

Charles's law states that:

The local weather forecaster reports that the current barometric pressure is 30.4 inches of mercury.What is the current pressure in atmospheres?

A gas sample is held at constant pressure.The gas occupies 3.62 L of volume when the temperature is 21.6°C.Determine the temperature at which the volume of the gas is 3.42 L.

Boyle's law states that:

Consider a sample of gas in a container on a comfortable spring day.The Celsius temperature suddenly doubles,and you transfer the gas to a container with twice the volume of the first container.If the original pressure was 12 atm,what is a good estimate for the new pressure?

Which of the following would represent the greatest pressure?

A physics experiment is conducted at a pressure of 14.4 kPa.What is this pressure in mmHg?

Pressure is

A balloon has a volume of 2.32 liters at 24.0°C.The balloon is heated to 48.0°C.Calculate the new volume of the balloon.

Gaseous chlorine is held in two separate containers at identical temperature and pressure.The volume of container 1 is 1.30 L,and it contains 6.70 mol of the gas.The volume of container 2 is 2.33 L.How many moles of the gas are in container 2?

The SI unit of pressure is the

The air pressure in the inner tube of a tire on a typical racing bike is held at a pressure of about 112 psi.Convert this pressure to atm.

Avogadro's law states that:

Body temperature is about 309 K.On a cold day,what volume of air at 276 K must a person with a lung capacity of 2.2 L breathe in to fill the lungs?