Medium
Write the applications of equilibrium constants.
(N/A) The equilibrium constant $(K)$ provides valuable information about a chemical reaction:
$1$. Predicting the extent of a reaction: If $K_c > 10^3$,the product predominates; if $K_c < 10^{-3}$,the reactant predominates; if $K_c$ is between $10^{-3}$ and $10^3$,both reactants and products are present in significant amounts.
$2$. Predicting the direction of the reaction: By comparing the reaction quotient $(Q_c)$ with the equilibrium constant $(K_c)$: if $Q_c < K_c$,the reaction proceeds in the forward direction; if $Q_c > K_c$,it proceeds in the reverse direction; if $Q_c = K_c$,the system is at equilibrium.
$3$. Calculating equilibrium concentrations: Given the initial concentrations and the value of $K_c$,the equilibrium concentrations of reactants and products can be calculated.
$1$. Predicting the extent of a reaction: If $K_c > 10^3$,the product predominates; if $K_c < 10^{-3}$,the reactant predominates; if $K_c$ is between $10^{-3}$ and $10^3$,both reactants and products are present in significant amounts.
$2$. Predicting the direction of the reaction: By comparing the reaction quotient $(Q_c)$ with the equilibrium constant $(K_c)$: if $Q_c < K_c$,the reaction proceeds in the forward direction; if $Q_c > K_c$,it proceeds in the reverse direction; if $Q_c = K_c$,the system is at equilibrium.
$3$. Calculating equilibrium concentrations: Given the initial concentrations and the value of $K_c$,the equilibrium concentrations of reactants and products can be calculated.
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Similar Questions
$A$ sample of pure $PCl_{5}$ was introduced into an evacuated vessel at $473 \, K$. After equilibrium was attained,the concentration of $PCl_{5}$ was found to be $0.5 \times 10^{-1} \, mol \, L^{-1}$. If the value of $K_{c}$ is $8.3 \times 10^{-3}$,what are the concentrations of $PCl_{3}$ and $Cl_{2}$ at equilibrium?
$PCl_{5(g)} \longleftrightarrow PCl_{3(g)} + Cl_{2(g)}$
$PCl_{5(g)} \longleftrightarrow PCl_{3(g)} + Cl_{2(g)}$
Medium
View SolutionFor the reaction $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$,the equilibrium constant $K_p$ is $16$. If the volume of the container is reduced to $\frac{1}{2}$ of its original value,what will be the value of $K_p$ at the same temperature?
Medium
View SolutionIf the equilibrium constant for the reaction $2AB \rightleftharpoons A_2 + B_2$ is $49$,what is the equilibrium constant for $AB \rightleftharpoons \frac{1}{2}A_2 + \frac{1}{2}B_2$?
Equilibrium constant,$K_{c}$ for the reaction $N_{2(g)} + 3H_{2(g)} \longleftrightarrow 2NH_{3(g)}$ at $500 \, K$ is $0.061$. At a particular time,the analysis shows that the composition of the reaction mixture is $[N_{2}] = 3.0 \, mol \, L^{-1}$,$[H_{2}] = 2.0 \, mol \, L^{-1}$,and $[NH_{3}] = 0.5 \, mol \, L^{-1}$. Is the reaction at equilibrium? If not,in which direction does the reaction tend to proceed to reach equilibrium?
Medium
View SolutionConsider the following gaseous equilibria with equilibrium constants $K_{1}$ and $K_{2}$ respectively:
$SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)}$
$2 SO_{3(g)} \rightleftharpoons 2 SO_{2(g)} + O_{2(g)}$
The equilibrium constants are related as:
$SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)}$
$2 SO_{3(g)} \rightleftharpoons 2 SO_{2(g)} + O_{2(g)}$
The equilibrium constants are related as:
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