Question 1

A gas sample originally occupies 436 mL at 24 °C.When the volume is expanded to 612 mL and the temperature is increased to 97 °C,the pressure becomes 526 mm Hg.What was the original pressure?
A)183 mm Hg
B)301 mm Hg
C)467 mm Hg
D)593 mm Hg
E)920 mm Hg

Accepted Answer

The answer of A gas sample originally occupies 436 mL...

Question 2

The pressure of the gas in a compressed gas tank is 862 kPa when the gas is at 35 °C.To what will the pressure change when the temperature drops to 7 °C? A)0.00128 kPa B)4.31 × 10³ kPa C)172 kPa D)784 kPa E)948 kPa

Accepted Answer

The pressure change can be calculated using the ideal gas law, assuming the volume and the amount of gas remain constant. The formula to use is $ P_1/T_1 = P_2/T_2 $, where $ P $ is pressure, $ T $ is temperature in Kelvin, and subscripts 1 and 2 refer to initial and final states, respectively. Convert temperatures to Kelvin: $ T_1 = 35 + 273 = 308 K $ and $ T_2 = 7 + 273 = 280 K $. Solve for $ P_2 $: $ P_2 = P_1 \times (T_2/T_1) = 862 \times (280/308) = 784 kPa $.

Question 3

A canister holds a gas at 16.3 psi when the temperature is -15 °C.What will the pressure be when the temperature is increased to 20.°C?
A)-12.2 psi
B)-21.7 psi
C)21.7 psi
D)14.4 psi
E)18.5 psi

Accepted Answer

To find the new pressure after a temperature change, we can use the combined gas law, which simplifies to $P_1/T_1 = P_2/T_2$ when the volume and amount of gas are constant. First, convert temperatures to Kelvin: $T_1 = -15°C + 273.15 = 258.15 K$ and $T_2 = 20°C + 273.15 = 293.15 K$. Solve for $P_2$: $P_2 = P_1 \times (T_2/T_1) = 16.3 \times (293.15/258.15) ≈ 18.5 psi$.

Question 4

The STP volume of an ideal gas is 2.06 m³.Calculate the volume of the sample at 1.75 atm and 27 °C. A)0.773 m³ B)1.07 m³ C)1.29 m³ D)3.28 m³ E)3.96 m³

Accepted Answer

The answer of The STP volume of an ideal gas...

Question 5

A scientist builds a "pressure thermometer" by sealing air in a tank.If the pressure inside the tank is 946 mm Hg when it is placed in a boiling water bath at 99 °C,and 749 mm Hg when left on the laboratory bench,what is the temperature in the lab?
A)295 °C
B)197 °C
C)125 °C
D)78 °C
E)22 °C

Accepted Answer

This problem can be solved using the Gay-Lussac's Law of Pressure-Temperature, which states that the pressure of a gas is directly proportional to its temperature in kelvins. The formula is $ P_1/T_1 = P_2/T_2 $, where $ P_1 $ and $ P_2 $ are the pressures at temperatures $ T_1 $ and $ T_2 $, respectively. Given $ P_1 = 946 $ mm Hg at $ T_1 = 99 $ °C (which is 372 K, since you add 273 to convert Celsius to Kelvin) and $ P_2 = 749 $ mm Hg, we need to find $ T_2 $ in °C.Rearranging the formula to solve for $ T_2 $, we get $ T_2 = T_1 \times (P_2 / P_1) $. Plugging in the numbers: $ T_2 = 372 \times (749 / 946) $ gives $ T_2 $ in Kelvin. Converting the result back to Celsius by subtracting 273 will give the temperature in the lab, which is approximately 22 °C.

Question 6

Calculate the original volume of a sealed balloon if it was originally at 25 °C and 1.02 atm,and then it was changed to 5.79 L,77 °C,and 1.72 atm.
A)4.03 L
B)3.17 L
C)8.31 L
D)2.92 L
E)11.5 L

Accepted Answer

The answer of Calculate the original volume of a sealed...

Question 7

A gas occupies 4.71 liters at 62 °C and 795 torr.What volume will it occupy if it is cooled to 17 °C and compressed to 911 torr?
A)3.56 L
B)6.23 L
C)1.13 L
D)4.75 L
E)4.67 L

Accepted Answer

To solve this problem, we use the combined gas law, which is $P_1V_1/T_1 = P_2V_2/T_2$, where $P$ is pressure, $V$ is volume, and $T$ is temperature in Kelvin. First, convert temperatures to Kelvin: $62 °C = 335 K$ and $17 °C = 290 K$. Then, plug in the given values and solve for $V_2$: $795 \text{ torr} \times 4.71 \text{ L} / 335 \text{ K} = 911 \text{ torr} \times V_2 / 290 \text{ K}$. Solving for $V_2$ gives approximately $3.56 L$.

Question 8

A gas sample is originally at 93.9 kPa and 27 °C with a volume of 1.17 m³.What will be the resulting temperature if the pressure is adjusted to 117 kPa and the volume is reduced to 0.730 m³? A)326 °C B)113 °C C)21 °C D)-123 °C E)-40 °C

Accepted Answer

Using the combined gas law, the resulting temperature is calculated to be approximately 233 K, which is -40 °C.

Question 9

A gas storage tank holds a gas at 5.73 atm pressure at 22 °C.What will the pressure of the gas be when the temperature is lowered to 0 °C?
A)5.30 atm
B)6.19 atm
C)0.189 atm
D)0 atm
E)The temperature of a gas at 0 °C is undefined

Accepted Answer

We can use the combined gas law which states that P1V1/T1 = P2V2/T2. We can assume that the volume remains constant, so V1 = V2. We can also assume that the amount of gas remains constant, so we can cancel out the V's. Rearranging the formula gives us P2 = (P1*T2)/T1. Plugging in the given values, we get P2 = (5.73 atm * 273 K)/(295 K) = 5.30 atm.

Question 10

A fixed quantity of a gas is maintained at a constant temperature.The gas has a volume of 0.847 m³ at 735 torr.What is the pressure of the gas when the volume is changed to 0.905 m³? A)0.00145 torr B)0.00127 torr C)781 torr D)563 torr E)688 torr

Accepted Answer

According to Boyle's Law (P1V1 = P2V2), the pressure and volume of a gas are inversely proportional at constant temperature. Using the initial conditions (P1 = 735 torr, V1 = 0.847 m³) and the final volume (V2 = 0.905 m³), we can solve for the final pressure (P2): P2 = (P1 * V1) / V2 = (735 torr * 0.847 m³) / 0.905 m³ = 688 torr.

Question 11

The pressure of a gas is 817 torr at 55.0°C.The quantity of the gas is fixed and the volume remains constant as the pressure is adjusted to 6.00 × 10² torr.What is the resulting temperature of the gas? A)-32 °C B)40 °C C)174 °C D)241 °C E)447 °C

Accepted Answer

Using the combined gas law, we can solve for the final temperature:P1/T1 = P2/T2817 torr / (55.0°C + 273.15) = 6.00 × 10^2 torr / (T2 + 273.15)T2 = 241 °C

Question 12

20.0 L of a gas originally at 22 °C and 1.05 atm pressure are compressed to 10.0 L.The new temperature is 57 °C.What is the new pressure?
A)2.35 atm
B)5.44 atm
C)0.469 atm
D)1.88 atm
E)0.587 atm

Accepted Answer

Using the combined gas law, $P_1V_1/T_1 = P_2V_2/T_2$, where $P$ is pressure, $V$ is volume, and $T$ is temperature in Kelvin. Convert temperatures to Kelvin: $T_1 = 22°C + 273 = 295K$ and $T_2 = 57°C + 273 = 330K$. Solve for $P_2$: $P_2 = P_1V_1T_2 / (V_2T_1) = (1.05 atm)(20.0 L)(330K) / (10.0 L)(295K) ≈ 2.35 atm$.

Question 13

A gas sample occupies 8.15 volume units at 677 pressure units.If possible,find the volume of the gas if the pressure is changed to 278 pressure units.The pressure units are the same in both cases and the temperature is constant.
A)It is not possible to find the new volume, although it would be greater than the original volume.
B)It is not possible to find the new volume, although it would be less than the original volume.
C)It is not possible to find the new volume, and no comparison with the original volume is possible.
D)19.8 volume units
E)3.35 volume units

Accepted Answer

This problem can be solved using Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature (P1V1 = P2V2). Given P1 = 677 pressure units, V1 = 8.15 volume units, and P2 = 278 pressure units, we can solve for V2: V2 = (P1V1)/P2 = (677 * 8.15) / 278 = 19.8 volume units.

Question 14

4.27 L of a gas are collected at 53 °C and 527 torr.What would this volume be if adjusted to STP?
A)0 L
B)7.35 L
C)5.16 L
D)3.54 L
E)2.48 L

Accepted Answer

The answer of 4.27 L of a gas are collected...

Question 15

A gas occupies a volume of 3.5 L at 24 °C and 883 mm Hg.What volume will it occupy at STP?
A)2.7 L
B)3.3 L
C)3.7 L
D)4.4 L
E)7.0 L

Accepted Answer

The answer of A gas occupies a volume of 3.5...

Question 16

A gas is collected in a container of fixed volume at 25 °C.If the gas exerts a pressure of 685 mm Hg at this temperature,what will the temperature of the gas be when the pressure is 7.60 × 10² mm Hg? A)331 °C B)58 °C C)28 °C D)23 °C E)-4 °C

Accepted Answer

Using Gay-Lussac's Law (P1/T1 = P2/T2), convert temperatures to Kelvin, solve for T2, and convert back to Celsius. T2 = 331 K, which is 58 °C.

Quiz 4: Introduction to Gases

A gas sample originally occupies 436 mL at 24 °C.When the volume is expanded to 612 mL and the temperature is increased to 97 °C,the pressure becomes 526 mm Hg.What was the original pressure?

The pressure of the gas in a compressed gas tank is 862 kPa when the gas is at 35 °C.To what will the pressure change when the temperature drops to 7 °C?

A canister holds a gas at 16.3 psi when the temperature is -15 °C.What will the pressure be when the temperature is increased to 20.°C?

The STP volume of an ideal gas is 2.06 m3.Calculate the volume of the sample at 1.75 atm and 27 °C.

A scientist builds a "pressure thermometer" by sealing air in a tank.If the pressure inside the tank is 946 mm Hg when it is placed in a boiling water bath at 99 °C,and 749 mm Hg when left on the laboratory bench,what is the temperature in the lab?

Calculate the original volume of a sealed balloon if it was originally at 25 °C and 1.02 atm,and then it was changed to 5.79 L,77 °C,and 1.72 atm.

A gas occupies 4.71 liters at 62 °C and 795 torr.What volume will it occupy if it is cooled to 17 °C and compressed to 911 torr?

A gas sample is originally at 93.9 kPa and 27 °C with a volume of 1.17 m3.What will be the resulting temperature if the pressure is adjusted to 117 kPa and the volume is reduced to 0.730 m3?

A gas storage tank holds a gas at 5.73 atm pressure at 22 °C.What will the pressure of the gas be when the temperature is lowered to 0 °C?

A fixed quantity of a gas is maintained at a constant temperature.The gas has a volume of 0.847 m3 at 735 torr.What is the pressure of the gas when the volume is changed to 0.905 m3?

The pressure of a gas is 817 torr at 55.0°C.The quantity of the gas is fixed and the volume remains constant as the pressure is adjusted to 6.00 × 102 torr.What is the resulting temperature of the gas?

20.0 L of a gas originally at 22 °C and 1.05 atm pressure are compressed to 10.0 L.The new temperature is 57 °C.What is the new pressure?

A gas sample occupies 8.15 volume units at 677 pressure units.If possible,find the volume of the gas if the pressure is changed to 278 pressure units.The pressure units are the same in both cases and the temperature is constant.

4.27 L of a gas are collected at 53 °C and 527 torr.What would this volume be if adjusted to STP?

A gas occupies a volume of 3.5 L at 24 °C and 883 mm Hg.What volume will it occupy at STP?

A gas is collected in a container of fixed volume at 25 °C.If the gas exerts a pressure of 685 mm Hg at this temperature,what will the temperature of the gas be when the pressure is 7.60 × 102 mm Hg?

The STP volume of an ideal gas is 2.06 m³.Calculate the volume of the sample at 1.75 atm and 27 °C.

A gas sample is originally at 93.9 kPa and 27 °C with a volume of 1.17 m³.What will be the resulting temperature if the pressure is adjusted to 117 kPa and the volume is reduced to 0.730 m³?

A fixed quantity of a gas is maintained at a constant temperature.The gas has a volume of 0.847 m³ at 735 torr.What is the pressure of the gas when the volume is changed to 0.905 m³?

The pressure of a gas is 817 torr at 55.0°C.The quantity of the gas is fixed and the volume remains constant as the pressure is adjusted to 6.00 × 10² torr.What is the resulting temperature of the gas?

A gas is collected in a container of fixed volume at 25 °C.If the gas exerts a pressure of 685 mm Hg at this temperature,what will the temperature of the gas be when the pressure is 7.60 × 10² mm Hg?