question_answer

The reaction, \[2A(g)+B(g)\rightleftharpoons 3C(g)+D(g)\] is begun with the concentration of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

A) \[[{{(0.75)}^{3}}(0.25)]\div [{{(1.00)}^{2}}(1.00)]\]

B) \[[{{(0.75)}^{3}}(0.25)]\div [{{(0.50)}^{2}}(0.75)]\]

C) \[[{{(0.75)}^{3}}(0.25)]\div [{{(0.50)}^{2}}(0.25)]\]

D) \[[{{(0.75)}^{3}}(0.25)]\div [{{(0.75)}^{2}}(0.25)]\]