What is the value of Kc for this equilibrium reaction?

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The equilibrium reaction involves N2O4 and NO2, with initial amounts of 1.0 mol each in a 1.0 dm3 vessel. At equilibrium, 0.75 mol of N2O4 remains, indicating that 0.25 mol has reacted. The correct calculation for Kc is derived from the equilibrium concentrations, leading to a value of 3.0. The initial misunderstanding in the calculation was clarified, confirming that the method used was appropriate. Understanding the equilibrium expression and the balanced chemical equation is crucial for solving such problems accurately.
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Homework Statement


A 1.0 dm3 reaction vessel contains initially 1.0 mol of N2O4(g) and 1.0 mol of NO2(g).
At equilibrium, 0.75mol of N2O4(g) are present.
What is the value of Kc?
A. 0.33
B. 0.50
C. 2.0
D. 3.0

The Attempt at a Solution


Right answer = D, but I do not why. My attempt for Kc is (3/4)^2 / (9/8) = 0.5, so wrong answer. Please, help me with this stricky one.
 

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Show the equilibrium equation in terms of the agents and also the actual balanced chemical equation.
 
GCT said:
Show the equilibrium equation in terms of the agents and also the actual balanced chemical equation.

Yes indeed. That is the right method to solve this.

Thank you!
 

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