chemistry question

Question

Consider the reaction.

2A(g)↽−−⇀B(g) 𝐾p=6.75×10−5 at 500 K

If a sample of A(g) at 2.00atm is heated to 500 K, what is the pressure of B(g) at equilibrium? 

Can someone show me the steps as well please.

Answer 1

One way to look at this is via an ICE table:

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

2.00atm........0 atm .......Initial

-2x...............+x..............Change

2.00-x............x..............Equilibrium

We can write the Kp expression as

Kp = (B) / (A)²

Plug in our values and solve for x...

6.75x10^-5 = (x) / (2-x)²

The rest is algebra and using the quadratic formula

Once you find x, that will be the equilibrium pressure of B