Problem: The reaction2NO(g) + Br2(g) ⇌ 2NOBr(g)has Kp = 109 at 25ºC. If the equilibrium partial pressure of Br 2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.

🤓 Based on our data, we think this question is relevant for Professor Hogan's class at LSU.

FREE Expert Solution
Problem Details

The reaction

2NO(g) + Br2(g) ⇌ 2NOBr(g)

has Kp = 109 at 25ºC. If the equilibrium partial pressure of Br 2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Equilibrium Expressions concept. If you need more Equilibrium Expressions practice, you can also practice Equilibrium Expressions practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hogan's class at LSU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.