1st Unit-7 Review_21

The partial pressures of CH₄, N₂, and O₂ in a sample of gas were found to be 135 mm Hg, 508 mm Hg, and 571 mm Hg, respectively. Calculate the mole fraction of nitrogen.

• 20.4

• 0.470

• 0.418

• 0.751

A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?

• 234 mmHg
• 1.37 mmHg
• 2.64 mmHg
• 1, 494 mmHg

Solid aluminum react with HCl according to the following balanced equation at STP:

2Al (s) + 6HCl (aq) --> 2AlCl₃ (aq) + 3H₂ (g)

If 13.5 g of Al (s) reacts with excess HCl, how many liters of H₂ gas are generated?

• 15.2 L

• 16.8 L

• 12.5 L

• 14.8 L

What are the standard temperature and pressure conditions for gases?

• 0 K and 760 mm Hg
• 273˚C and 1.0 atm
• 273 K and 101.3 kPa
• 0˚C and 760 kPa

A mixture of 2 moles of H₂, 3 moles of NH₃, 4 moles of CO₂, and 5 moles of N₂ exert a total pressure of 800. torr. What is the partial pressure of CO₂?

• 228 torr

• 114 torr

• 286 torr

• 160. torr

A sample of gas with a volume of 30.0 mL at 25.0^oC is heated to 50.0^oC.  What is the new volume of the gas?

• 60.0 mL
• 15.0 mL
• 27.5 mL
• 32.5 mL

Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa.

• -266 degrees C

• -622 degrees C

• 622 degrees C

• 266 degrees C

How many liters of NH₃ are needed to react completely with 30.0L of NO? At constant Temperature and Pressure!

4NH₃(g) + 6NO (l) --> 5N₂ (g) + 6H₂O (l)

• 5.0 L

• 20.0 L

• 7.5 L

• 120.0 L

In order to solve gas law calculations, temperature must be measured in:

• Fahrenheit
• Celsius
• Kelvin
• It doesn't matter 

Mg₃N_2(s) + 3H₂O_(l) ––> 3 MgO + 2NH_3(g)

If 10.3 g of magnesium nitride is used, what volume of ammonia gas would be collected at 20.0˚C and 0.989 atm?

• 27.1 L H₂

• 4.96 L H₂

• 0.204 L H₂

• 10.3 L H₂