Consider the reaction. 2A(g)↽−−⇀B(g)𝐾p=5.93×10−5at 500 K If a sample of A(g) at 3.10 atm is heated to 500 K, what is the pressure of B(g) at equilibrium?

Answer 1

2A(g) <===> B(g)

3.10................0......I

-2x.................+x.....C

3.1-2x..............x.....E

Kp = 5.93x10^-5 = (B)/(A)²

5.93x10^-5 = x / (3.1-2x)²

Because Kp is rather small (10^-5), we can ignore -2x to simplify the calculations:

5.93x10^-5 = x / (3.1)²

x = 5.7x10^-4 atm = partial pressure of B at equilibrium