(A) Initial: $[A_2] = 1 \ M, [B_2] = 0 \ M$ Equilibrium: $[A_2] = (1-x) \ M, [B_2] = x \ M$ $K_{c} = \frac{[B_2]}{[A_2]}$ $39 = \frac{x}{1-x}$ $39 - 3

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(A) Initial: $[A_2] = 1 \ M, [B_2] = 0 \ M$ Equilibrium: $[A_2] = (1-x) \ M, [B_2] = x \ M$ $K_{c} = \frac{[B_2]}{[A_2]}$ $39 = \frac{x}{1-x}$ $39 - 39x = x$ $40x = 39$ $x = \frac{39}{40} = 0.975$ $[B_2] = 0.975 \ M$ $[A_2] = 1 - 0.975 = 0.025 \ M$

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Easy

$K_{c}$ for the reaction $A_{2(g)} \rightleftharpoons B_{2(g)}$ is $39.0$. In a closed one litre flask,one mole of $A_{2(g)}$ was heated to $T \ K$. What are the concentrations of $A_{2(g)}$ and $B_{2(g)}$ (in $mol \ L^{-1}$) respectively at equilibrium?

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A
$0.025, 0.975$
B
$0.975, 0.025$
C
$0.05, 0.95$
D
$0.02, 0.98$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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$K_{c}$ for the reaction $A_{2(g)} \rightleftharpoons B_{2(g)}$ is $39.0$. In a closed one litre flask,one mole of $A_{2(g)}$ was heated to $T \ K$. What are the concentrations of $A_{2(g)}$ and $B_{2(g)}$ (in $mol \ L^{-1}$) respectively at equilibrium?

Similar Questions

In a chemical equilibrium,the rate constant of the backward reaction is $7.5 \times 10^{-4}$ and the equilibrium constant is $1.5$. The rate constant of the forward reaction is:

$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$The reaction was started with some amount of $NH_4HS$. The equilibrium pressure at $25^{\circ}C$ is $0.5 \ atm$. What is $K_p$ for the reaction (in $atm^2$)?

$40\%$ of $HI$ undergoes decomposition to $H_2$ and $I_2$ at $300 \ K$. $\Delta G^{\ominus}$ for this decomposition reaction at one atmosphere pressure is $... \ J \ mol^{-1}$. [nearest integer](Use $R = 8.31 \ J \ K^{-1} \ mol^{-1}$; $\log 2 = 0.3010$; $\ln 10 = 2.3$; $\log 3 = 0.477$)

Given below are certain reactions. Identify the reaction for which $K_p = K_c$.

$8 \ mol$ of $AB_3$ is taken in a $1.0 \ dm^3$ container. It dissociates according to the reaction $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$. If $2 \ mol$ of $A_2$ are present at equilibrium,the equilibrium constant $K_c$ of the reaction is ....... $mol^2 \ L^{-2}$.

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$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$
The reaction was started with some amount of $NH_4HS$. The equilibrium pressure at $25^{\circ}C$ is $0.5 \ atm$. What is $K_p$ for the reaction (in $atm^2$)?

$40\%$ of $HI$ undergoes decomposition to $H_2$ and $I_2$ at $300 \ K$. $\Delta G^{\ominus}$ for this decomposition reaction at one atmosphere pressure is $... \ J \ mol^{-1}$. [nearest integer]
(Use $R = 8.31 \ J \ K^{-1} \ mol^{-1}$; $\log 2 = 0.3010$; $\ln 10 = 2.3$; $\log 3 = 0.477$)