In this lesson, we will learn how to construct and calculate the equilibrium constant for partial pressures.

Students will be able to

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 20.00% at 298 K, as shown:

NO2NO242

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

Q3:

6.00 mol of N2 gas and 20.00 mol of H2 were allowed to react at 650 K and 50 atm of pressure. At equilibrium, 4 mol of N2 gas had been converted into ammonia according to the following reaction equation:

N()+3H()2NH()223ggg

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

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