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When the compound A2X(g) is placed in a flask at 1200 degrees C, it dissociates into A2(g) and X2(g) as shown in the following equation:

2A2X(g)<----->2A2(g) + X2(g)

If the initial concentration of A2X is 2.00 M and 15.0% of the A2X vapor is dissociated when equilibrium is reached, what is the value of the equilibrium constant for the reaction?

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