Question 1

Which is not a property of a gas?
A)The density of a gaseous substance varies strongly with temperature.
B)A sample of gas assumes the shape and volume of its container.
C)Gases are highly compressible.
D)The densities of gases are much larger than those of corresponding liquids.
E)Gases form homogeneous mixtures with one another in any proportion.

Accepted Answer

The densities of gases are much smaller than those of corresponding liquids.

Question 2

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×10⁵ Pa = 760 torr) A)0.217 atm B)0.466 atm C)0.613 atm D)1.63 atm E)4.60 atm

Accepted Answer

To convert from torr to atm, we need to divide by 760 torr/1 atm:
466 torr ÷ 760 torr/1 atm = 0.613 atm. Therefore, the pressure in atmospheres is 0.613 atm.

Question 3

Which of the following is/are characteristic(s)of gases?
A)High compressibility
B)Relatively large distances between molecules
C)Formation of homogeneous mixtures regardless of the nature of gases
D)Choice 1 and 2 only
E)Choice 1,2,and 3

Accepted Answer

A) Gases can be easily compressed due to the large distances between molecules.
B) In gases, molecules are relatively far apart from each other. This increases the free space for movement of gas particles, leading to low density.
C) In gases, the mixtures are homogeneous, and the molecules of different types of gases are uniformly distributed. Therefore, regardless of the nature of gases, they form homogeneous mixtures.

Question 4

The air pressure in a volleyball is 75 psi.What is this pressure in torr? (1 atm = 14.7 psi =101,325 Pa = 760 torr)?
A)520 torr
B)562 torr
C)3900 torr
D)7600 torr
E)75,000 torr

Accepted Answer

The answer of The air pressure in a volleyball is...

Question 5

If the atmospheric pressure in Denver is 0.8800 atm,what is this pressure expressed in mmHg? (1 atm = 101,325 Pa = 760 torr,1 torr = 1 mmHg)? A)151.5 mmHg B)1.16 × 10^-3 mmHg C)863.6 mmHg D)8.92 × 10⁴ mmHg E)668.8 mmHg

Accepted Answer

To convert atmospheric pressure from atm to mmHg, we need to multiply by the conversion factor of 760 mmHg/1 atm. Therefore, atmospheric pressure in mmHg is:
0.8800 atm x 760 mmHg/1 atm = 668.8 mmHg. Thus, the answer is (E).

Question 6

"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ law.
A)Charles's
B)Boyle's
C)Amontons's
D)Avogadro's
E)Gay-Lussac's

Accepted Answer

This statement represents Boyle's law, which relates the pressure and volume of an ideal gas at constant temperature and number of moles. Charles's law relates the volume and temperature of an ideal gas at constant pressure and number of moles. Amontons's law relates the temperature and pressure of an ideal gas at constant volume and number of moles. Avogadro's law relates the volume and number of moles of an ideal gas at constant temperature and pressure. Gay-Lussac's law relates the pressure and temperature of an ideal gas at constant volume and number of moles.

Question 7

What is the pressure in atmospheres exerted by a column of water that is 12.5 m high? (density of water = 1.00g/cm³; gravitational constant = 9.80665 m/s²,1 atm = 101,325 Pa = 760 torr = 760 mmHg) A)123 atm B)1.23 × 10⁵ atm C)0.785 atm D)1.21 atm E)1.23 × 10^-3 atm

Accepted Answer

To find the pressure exerted by a column of water, use the formula P = ρgh, where ρ is the density of water (1000 kg/m³, converting from 1.00 g/cm³), g is the acceleration due to gravity (9.80665 m/s²), and h is the height of the water column (12.5 m). Substituting these values gives P = 1000 kg/m³ * 9.80665 m/s² * 12.5 m = 122583.125 Pa. Converting this to atmospheres (since 1 atm = 101325 Pa), P = 122583.125 Pa / 101325 Pa/atm ≈ 1.21 atm.

Question 8

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L.What volume will it occupy if the pressure is increased to 894 torr at constant temperature?
A)22.3 L
B)31.2 L
C)44.9 L
D)112 L
E)380 L

Accepted Answer

The answer of A sample of nitrogen gas at 298...

Question 9

"The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure" is a statement of _____________ law.
A)Charles's
B)Boyle's
C)Dalton's
D)Avogadro's
E)Gay-Lussac's

Accepted Answer

Avogadro's law states that the volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure. This law is derived from experiments and helps to explain the behavior of gases.

Question 10

A flask containing argon gas is connected to a closed-ended mercury manometer.The closed end is under vacuum.If the mercury level in the closed arm is 230.mm above that in the arm connected to the flask,what is the argon pressure,in torr?
A)-230.torr
B)230.torr
C)530.torr
D)790.torr
E)990.torr

Accepted Answer

The argon pressure is equal to the difference in mercury levels, which is 230 mm. Since mercury's density directly translates to pressure in a manometer, and 1 mm of mercury equals 1 torr, the argon pressure is 230 torr.

Question 11

The pressure of sulfur dioxide in a container is 159 kPa.What is this pressure in atmospheres? (1 atm = 101,325 Pa = 760 torr)? A)0.209 atm B)0.637 atm C)1.57 atm D)21.2 atm E)1.59 ×10⁴ atm

Accepted Answer

The answer of The pressure of sulfur dioxide in a...

Question 12

A flask containing neon gas is connected to an open-ended mercury manometer.The open end is exposed to the atmosphere,where the prevailing pressure is 745 torr.The mercury level in the open arm is 5.0 cm below that in the arm connected to the flask of neon.What is the neon pressure,in torr?
A)-50.torr
B)50.torr
C)695 torr
D)745 torr
E)795 torr

Accepted Answer

The difference in height between the two arms of the manometer is equal to the difference between the pressures inside and outside the flask. Since the open-end is exposed to atmospheric pressure, we can calculate the pressure of the neon gas in the flask as follows:

Neon pressure = atmospheric pressure - pressure difference
Neon pressure = 745 torr - (5.0 cm x 13.6 torr/cm)  [1 mmHg = 1 torr, and density of mercury = 13.6 g/cm³]
Neon pressure = 695 torr

Therefore, the neon pressure in the flask is 695 torr.

Question 13

The pressure of hydrogen sulfide gas in a container is 3.565 ×10⁴ Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)? A)46.91 torr B)267.4 torr C)351.8 torr D)3612 torr E)2.709 ×10⁴ torr

Accepted Answer

To convert from Pa to torr, we need to use the conversion factor:
1 atm = 101,325 Pa = 760 torr

Therefore, we can set up the following dimensional analysis:
3.565 × 10^14 Pa x (760 torr/101,325 Pa) = 267.4 torr

Therefore, the pressure of hydrogen sulfide gas in torr is 267.4 torr.

Question 14

What is the formula which describes the relationship between the pressure and volume at constant temperature and constant number of moles? A)PV = k₁ B)V/P = k₁ C)P/V = k₁ D)k₁P = V E)P = -k₁V

Accepted Answer

The formula that describes the relationship between the pressure and volume at constant temperature and constant number of moles is Boyle's Law, which is represented as PV = k, where P is the pressure, V is the volume, and k is a constant.

Question 15

Which represents the definition of pressure?
A)volume/density
B)temperature × area
C)moles/volume
D)force/area
E)volume × force

Accepted Answer

Pressure is defined as force per unit area. Therefore, the correct formula to calculate pressure is force/area.

Question 16

A sample of a gas has an initial pressure of 0.987 atm and a volume of 12.8 L.What is the final pressure if the volume is increased to 25.6 L?
A)2.03 atm
B)1.97 atm
C)0.494 atm
D)0.003 atm
E)323.4 atm

Accepted Answer

According to Boyle's Law, at constant temperature, the product of pressure and volume is constant. P₁V₁ = P₂V₂. We can rearrange this equation to solve for the final pressure: 
P₂ = (P₁V₁)/V₂. 
Plugging in the values, we get P₂ = (0.987 atm x 12.8 L)/25.6 L = 0.494 atm. Therefore, the final pressure is 0.494 atm, which is choice C.

Question 17

A sample of an ideal gas has its volume doubled while its temperature remains constant.If the original pressure was 100 torr,what is the new pressure?
A)10 torr
B)50 torr
C)100 torr
D)200 torr
E)1000 torr

Accepted Answer

According to Charles's law, if the temperature of an ideal gas remains constant, the volume of the gas is directly proportional to its pressure. In this case, since the volume is doubled, the pressure must be halved to keep the temperature constant. Therefore, the new pressure would be 100/2 = 50 torr.

Question 18

A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm³; the density of water is 1.00 g/cm³. A)348 cm B)1.00 × 10² ft C)18.8 mm D)33.8 ft E)76.0 cm

Accepted Answer

The pressure exerted by a column of fluid is given by $P = h \cdot \rho \cdot g$, where $P$ is the pressure, $h$ is the height of the fluid column, $\rho$ is the density of the fluid, and $g$ is the acceleration due to gravity. Since the pressure is constant, we can set the pressures equal for mercury and water to find the height of the water column that would exert the same pressure as a 256 mm column of mercury. Given the density of mercury is 13.6 times that of water, the height of the water column will be 13.6 times 256 mm, or 3488 mm, which is 348 cm.

Question 19

What is the pressure in atmospheres exerted by a column of mercury that is 100.m high? (density of mercury = 13.5951 g/cm³,gravitational constant = 9.80665 m/s²,1 atm = 101,325 Pa = 760 torr = 760 mmHg) A)1.4 × 10¹⁰ atm B)0.013 atm C)0.73 atm D)1.37 atm E)132 atm

Accepted Answer

The answer of What is the pressure in atmospheres exerted...

Question 20

"The volume of an ideal gas is directly proportional to its absolute temperature at constant pressure and number of moles" is a statement of ________________ law.
A)Charles's
B)Boyle's
C)Dalton's
D)Avogadro's
E)Gay-Lussac's

Accepted Answer

The statement given describes Charles's law, which states that the volume of a gas is directly proportional to its absolute temperature at constant pressure and number of moles.

Quiz 10: Gases

Which is not a property of a gas?

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×10⁵ Pa = 760 torr)

Which of the following is/are characteristic(s) of gases?

The air pressure in a volleyball is 75 psi.What is this pressure in torr? (1 atm = 14.7 psi =101,325 Pa = 760 torr) ?

If the atmospheric pressure in Denver is 0.8800 atm,what is this pressure expressed in mmHg? (1 atm = 101,325 Pa = 760 torr,1 torr = 1 mmHg) ?

"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ law.

What is the pressure in atmospheres exerted by a column of water that is 12.5 m high? (density of water = 1.00g/cm³; gravitational constant = 9.80665 m/s²,1 atm = 101,325 Pa = 760 torr = 760 mmHg)

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L.What volume will it occupy if the pressure is increased to 894 torr at constant temperature?

"The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure" is a statement of _____________ law.

A flask containing argon gas is connected to a closed-ended mercury manometer.The closed end is under vacuum.If the mercury level in the closed arm is 230.mm above that in the arm connected to the flask,what is the argon pressure,in torr?

The pressure of sulfur dioxide in a container is 159 kPa.What is this pressure in atmospheres? (1 atm = 101,325 Pa = 760 torr) ?

A flask containing neon gas is connected to an open-ended mercury manometer.The open end is exposed to the atmosphere,where the prevailing pressure is 745 torr.The mercury level in the open arm is 5.0 cm below that in the arm connected to the flask of neon.What is the neon pressure,in torr?

The pressure of hydrogen sulfide gas in a container is 3.565 ×10⁴ Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr) ?

What is the formula which describes the relationship between the pressure and volume at constant temperature and constant number of moles?

Which represents the definition of pressure?

A sample of a gas has an initial pressure of 0.987 atm and a volume of 12.8 L.What is the final pressure if the volume is increased to 25.6 L?

A sample of an ideal gas has its volume doubled while its temperature remains constant.If the original pressure was 100 torr,what is the new pressure?

A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm³; the density of water is 1.00 g/cm³.

What is the pressure in atmospheres exerted by a column of mercury that is 100.m high? (density of mercury = 13.5951 g/cm³,gravitational constant = 9.80665 m/s²,1 atm = 101,325 Pa = 760 torr = 760 mmHg)

"The volume of an ideal gas is directly proportional to its absolute temperature at constant pressure and number of moles" is a statement of ________________ law.