Equilibrium constant?

Question

N2(g) + 3 Cl2(g) 2 NCl3(g)

An equilibrium mixture of this reaction at a certain temperature was found to have [NCl3] = 1.9x10^-1 M, [N2] = 1.4x10^-3 M, and [Cl2] = 4.3x10^-4 M. What is the value of the equilibrium constant at this temperature?

My answer is 3.08x10^12. Can anyone tell me why this is wrong?

(1.4x10^-3)(4.3x10^-4)^3

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(1.9x10^-1)^2

Is my problem not set up correctly?

Answer 1

I believe that the 'product' goes on top and the reactants on bottom.

So in essence,

you've flipped the equation and it should be

(1.9x 10^-1)^2

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(1.4x10^-3)(4.3x10^-4)^3

See if this helps!!