Medium
At $298 \ K$,the $K_c$ of the reaction $Cu(s) + 2Ag^+(aq) \rightleftharpoons Cu^{2+}(aq) + 2Ag(s)$ is $3.0 \times 10^{14}$. In a reaction mixture at a certain temperature,$[Cu^{2+}] = 1.8 \times 10^{-2} \ M$ and $[Ag^+] = 3.0 \times 10^{-9} \ M$. Is this reaction in equilibrium? In which direction will the reaction proceed?
(B) The reaction quotient $Q_c$ is calculated as: $Q_c = \frac{[Cu^{2+}]}{[Ag^+]^2} = \frac{1.8 \times 10^{-2}}{(3.0 \times 10^{-9})^2} = \frac{1.8 \times 10^{-2}}{9.0 \times 10^{-18}} = 2.0 \times 10^{15}$.
Since $Q_c = 2.0 \times 10^{15}$ and $K_c = 3.0 \times 10^{14}$,we observe that $Q_c > K_c$.
Because $Q_c > K_c$,the reaction is not in equilibrium.
Since $Q_c > K_c$,the reaction will proceed in the reverse direction to reach equilibrium.
Since $Q_c = 2.0 \times 10^{15}$ and $K_c = 3.0 \times 10^{14}$,we observe that $Q_c > K_c$.
Because $Q_c > K_c$,the reaction is not in equilibrium.
Since $Q_c > K_c$,the reaction will proceed in the reverse direction to reach equilibrium.
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$A \rightleftharpoons B$ $K_C = 2$
$B \rightleftharpoons C$ $K_C = 3$
$C \rightleftharpoons D + E$ $K_C = 5$
$K_C$ for the reaction $A \rightleftharpoons D + E$ is:
$A \rightleftharpoons B$ $K_C = 2$
$B \rightleftharpoons C$ $K_C = 3$
$C \rightleftharpoons D + E$ $K_C = 5$
$K_C$ for the reaction $A \rightleftharpoons D + E$ is:
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View SolutionAt $T \ K$,the $K_C$ value for the reaction $\frac{1}{3} N_{2(g)} + H_{2(g)} \rightleftharpoons \frac{2}{3} NH_{3(g)}$ is $50$. The $K_C$ value for the reaction $2 NH_{3(g)} \rightleftharpoons N_{2(g)} + 3 H_{2(g)}$ at the same temperature is:
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At equilibrium,the concentrations of $N_{2} = 3.0 \times 10^{-3} \, M$,$O_{2} = 4.2 \times 10^{-3} \, M$ and $NO = 2.8 \times 10^{-3} \, M$ in a sealed vessel at $800 \, K$. What will be $K_{c}$ for the reaction
$N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$
$N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$
Medium
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