Chemistry PLS HELP

Question

Consider the reaction.

A(aq)↽−−⇀2B(aq)𝐾=3.04×10−6 at 500 K

If a 1.50 M sample of A is heated to 500 K, what is the concentration of B at equilibrium?

Answer 1

Set up an ICE table:

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

1.50.................0...........Initial

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

1.50-x.............2x..........Equilibrium

K = [B]²[A]

3.04x10^-6 = (2x)²(1.50-x) and because K is a low value, we can assume x is small and ignore it

3.04x10^-6 = (4x² )(1.50)

4x² =2.03x10^-6

x²= 5.07x10^-7

x = 7.12x10^-4 (which is small compared to 1.50 so the above assumption was valid)

[B] at equilibrium = 2x = (2)(7.12x10^-4) = 1.42x10^-3 M