QuestionMay 8, 2025

Nitrogen monoxide reacts with chlorine gas as follows: 2NO(g)+Cl_(2)(g)rightarrows 2NOCl(g) At 700 K. the equilibrium constant, K_(P) for this reaction is 0.26. Now, consider the following conditions at 700K:P(NO)=0.16atm,P(Cl_(2))=0.21atm and P(NOCl)=0.11atm Which of the following statements is true? A. The reaction proceeds forward towards the equilibrium B. The reaction proceeds in reverse towards the equilibrium C. The reaction is at equilibrium D. The rate of making products is faster than the rate of making reactants. E. Delta G=0

Nitrogen monoxide reacts with chlorine gas as follows: 2NO(g)+Cl_(2)(g)rightarrows 2NOCl(g) At 700 K. the equilibrium constant, K_(P) for this reaction is 0.26. Now, consider the following conditions at 700K:P(NO)=0.16atm,P(Cl_(2))=0.21atm and P(NOCl)=0.11atm Which of the following statements is true? A. The reaction proceeds forward towards the equilibrium B. The reaction proceeds in reverse towards the equilibrium C. The reaction is at equilibrium D. The rate of making products is faster than the rate of making reactants. E. Delta G=0
Nitrogen monoxide reacts with chlorine gas as follows: 2NO(g)+Cl_(2)(g)rightarrows 2NOCl(g) At 700 K. the equilibrium constant, K_(P) for this reaction is 0.26. Now, consider the following conditions at 700K:P(NO)=0.16atm,P(Cl_(2))=0.21atm and P(NOCl)=0.11atm Which of the following statements is true? A. The reaction proceeds forward towards the equilibrium B. The reaction proceeds in reverse towards the equilibrium C. The reaction is at equilibrium D. The rate of making products is faster than the rate of making reactants. E. Delta G=0

Solution
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Answer

B. The reaction proceeds in reverse towards the equilibrium Explanation 1. Calculate Reaction Quotient Q_P Use Q_P = \frac{(P_{NOCl})^2}{(P_{NO})^2 \cdot P_{Cl_2}}. Substitute values: Q_P = \frac{(0.11)^2}{(0.16)^2 \cdot 0.21}. 2. Compare Q_P with K_P Calculate Q_P: Q_P = \frac{0.0121}{0.005376} \approx 2.25. Since Q_P > K_P, the reaction proceeds in reverse.

Explanation

1. Calculate Reaction Quotient $Q_P$<br /> Use $Q_P = \frac{(P_{NOCl})^2}{(P_{NO})^2 \cdot P_{Cl_2}}$. Substitute values: $Q_P = \frac{(0.11)^2}{(0.16)^2 \cdot 0.21}$.<br />2. Compare $Q_P$ with $K_P$<br /> Calculate $Q_P$: $Q_P = \frac{0.0121}{0.005376} \approx 2.25$. Since $Q_P > K_P$, the reaction proceeds in reverse.
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