# Gas Laws

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## Gas Laws Answer Key

**Instructions:**
Read each question carefully. Choose the answer that best fits the question. Short answer response questions must be responded to in complete sentences. If the question involves calculations, you must show all your math work.

1.

Which equation is used in Boyle's Law calculations?

- [math]PV = "constant"[/math]
- [math](V)/(T) = "constant"[/math]
- [math](PV)/T = "constant"[/math]

2.

Which of the following equations represents the equation for the pressure of a real gas?

- [math]P={nRT}/{V-nb}[/math]
- [math]P={nRT}/{V-R}[/math]
- [math]P={nRT}/{V}[/math]
- [math]P={nRT}/{V-1}[/math]

3.

The equation for Dalton's Law of Partial Pressures is as follows: [math]"P"_"total" = P_1 + P_2 + ...[/math]. Write the result of a derivation for the pressure of an ideal gas, in terms of Dalton's Law of Partial Pressures.

- [math]"P"_"total" = (n_1 + n_2 + n_3 + n_4 + n_5 + ...)({RT}/V)[/math]

4.

What volume will 5.0 mol of Xe occupy at 50ºC and 1.27 atm of pressure? (R=0.0821 L•atm/mol•K)

- 16.2 L
- 104.4 L
- 0.0096 L
- 10.44 L

5.

What is the pressure of a 3.2-mol sample of helium gas that has a volume of 650 mL and that is present at a temperature of 500 K? (R=0.0821 L•atm/mol•K)

- 123705 atm
- 0.202 atm
- 123.71 atm
- 202.1 atm

6.

A sample of NO has a pressure of 66 mm Hg and a volume of 322 mL. When the NO is transferred to a 1.20-L flask, what is the pressure of the gas?

- 246 mm Hg
- 17.8 mm Hg
- 5855 mm Hg
- 17710 mm Hg

7.

A 1.35-L sample of gas exists at 355 K. When the gas is transferred to a 950-mL container at the same pressure, what is the temperature?

- 236.7 K
- 0.002 K
- 1.88 K
- 236666 K

8.

The particles of an ideal gas have strong attractive forces between them.

- True
- False

9.

A 2.0 liter container of nitrogen had a pressure of 3.2 atm. What volume would be necessary to decrease the pressure to 1.0 atm?

- [math]P_1V_1 = P_2V_2[/math]

[math](3.2atm)(2.0L)=(1.0atm)V_2[/math]

[math]P_2=((3.2atm)(2.0L))/(1.0atm)=6.4L[/math]

10.

A sample of helium has a volume of [math]521L[/math] at a pressure of [math]75cmHg[/math] and a temperature of [math]18degC[/math]. When the temperature is increased to [math]23degC[/math], what is the volume of the helium?

- Convert [math]degC" to "degK[/math]:

[math]T_1=18degC+273=291degK[/math]

[math]T_2=23degC+273=296degK[/math]

[math]V_2=(V_1T_2)/(T_1)=((521L)(296degK))/(291degK)=529.95L" or "530L[/math]

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