Optional gas laws quiz review

If 3.25 mol of Ar occupies 100. L at a particular temp and pressure, what volume (in L) will 14.15 mol of Ar occupy under same condition?

Enter your answer with the correct number of significant figures.

(a)  

What is the equation that relates moles and gas volume (Avogadro's Law)?

• P₁V₁ = P₂V₂

• PV = nRT

If 1.00 mol of He occupies 22.4 L at standard temperature and pressure (STP), what volume will 1.00 g of He occupy under the same conditions?

• 22.4 L
• 5.60 L
• 10.2 L
• 8.16 L

A balloon contains 0.504 moles of a gas at a volume of 2680 mL.  When the number of moles changes to 0.423 moles, what is the new volume of the balloon?

Enter your answer with the correct number of significant figures.

(a)  

A balloon containing 12.05 moles of a gas had an original volume of 265 L. If an additional 2.51 moles of the same gas are added at the same temperature and pressure, what is the new volume of the balloon?

• 0.662 L

• 55.2 L

• 320. L

• 1270 L

A balloon had an original volume of 12.05 L. Additional gas was added to the balloon. The new volume is 12.99 L when a total of 7.81 moles of gas are in the balloon. How many moles did the balloon originally contain?

• 20.04 mol

• 7.24 mol

• 1.53 mol

• 7.00 mol

A balloon contains 1.99 moles of a gas and has a volume of 12.2 L.

How many moles of this gas would occupy a volume of 15.6 L at the same conditions?

• 9.52 mol

• 2.55 mol

• 2.40 mol

• 7.41 mol

The pressure on a sample of gas is increased from 1.0 atm to 3.0 atm. If the new volume is 0.52 L, find the original volume.

• 0.52 L
• 1.56 L
• 0.173 L
• 1.00 L

If a beach ball has a volume of 261 L at a temperature of 502 K, what will be the new temperature of the balloon if the volume decreases to 176 L and the pressure remain constant?

• 744 K

• 0.0030 K

• 339 K

• 512 K

The pressure remains constant over a sample of helium gas occupying a volume of 638 mL. The temperature is increased to 471 K and the volume is now 953 mL. What was the original temperature?

• 315 K

• 1291 K

• 704 K

• 133 K