Lesson: The Equilibrium Constant for Partial Pressures Chemistry
In this lesson, we will learn how to construct and calculate the equilibrium constant for partial pressures.
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.
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.
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.