Consider the hypothetical reaction A(g)+2B(g)⇌ C(g)A(g) + 2B(g) ⇌ C(g)

Question

Consider the hypothetical reaction A(g)+2B(g)⇌ C(g)A(g) + 2B(g) ⇌ C(g)

If the equilibrium concentration of A is 0.000045 mol/L, of B is 0.02 mol/L, and of C is 0.0094 mol/L, what is K for the reaction?

a)0.22

b)2.3*10^8

c)4.3*10^5

d)none of these

Answer 1

I'm not sure that this equation is displaying correctly if the equation is:

A(g)+2B(g)⇌ C(g)

Keq = [C]¹/ ([A]*[B]²)

Keq = [0.0094] / ([0.000045]*[0.02]*[0.02])

Keq = 522222

Units... mol/L = M

M/ (M*M*M) = M/M³ = M^-2

Therefore Keq = 522222 (mol/L)^-2