# Lesson Worksheet: The Equilibrium Constant for Partial Pressures Chemistry

In this worksheet, we will practice constructing and calculating the equilibrium constant for partial pressures.

Q1:

A mixture of gases in a closed vessel at equilibrium contains three different gases: nitrogen (20 moles), hydrogen (45 moles), and ammonia (25 moles). Calculate the partial pressure of hydrogen at 40 atm.

Q2:

A sealed flask at a pressure of 1.50 atm contains dinitrogen tetroxide. The gas is found to have dissociated by at 298 K, as shown:

What is the value of the equilibrium constant, at 298 K? Give your answer to two decimal places.

Q3:

6.00 mol of gas and 20.00 mol of were allowed to react at 650 K and 50 atm of pressure. At equilibrium, 4 mol of gas had been converted into ammonia according to the following reaction equation:

Calculate for this equilibrium, giving your answer to two decimal places in scientific notation.

• A atm−2
• B atm−2
• C atm−2
• D atm−2
• E atm−2

Q4:

A mixture of gases at equilibrium contains 20 moles of gas, 40 moles of gas, and 40 moles of gas. What is the mole fraction of at equilibrium?

Q5:

If the value of at 900 K is 1.68 atm atm for the thermal decomposition of calcium carbonate, what is the partial pressure of carbon dioxide? Give your answer to two decimal places.

Q6:

A boat and its occupants floating on the surface of the sea are subject to a regular atmospheric pressure of 1 atm. A scuba diver dives off of the boat and swims downward. When the diver is 10 meters below the surface, the pressure is doubled. Use information from the pie chart to calculate the partial pressure of nitrogen 10 meters below the surface of the sea to two decimal places. Q7:

Consider the following equation:

Assuming that the pressures in a reaction between nitrogen and hydrogen to form ammonia are measured in atmospheres, what is the unit of the equation?

• Aatm−2
• Batm2
• Catm−1
• Datm−3
• Eatm

Q8:

The equilibrium of a mixture of gases can be evaluated by , the equilibrium constant for partial pressures.

Consider the following equation:

What is the correct equation of for the equilibrium between the two different oxides of nitrogen shown?

• A
• B
• C
• D
• E

Consider the following equation:

What is the correct equation of for the equilibrium between ammonia and oxygen shown?

• A
• B
• C
• D
• E

Q9:

The reaction

shows the thermal decomposition of lithium carbonate in a vacuum. Which of the following is the correct equation for ?

• A
• B
• C
• D
• E

Q10:

Choose the correct expression for the of the following reaction:

• A
• B
• C
• D
• E

This lesson includes 16 additional questions and 28 additional question variations for subscribers.