(C) The reaction is $A + B \rightleftharpoons C + D$.Species$A$$B$$C$$D$Initial moles$1$$1$$0$$0$Moles at equilibrium$(1-x)$$(1-x)$$x$$x$Given that at

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(C) The reaction is $A + B \rightleftharpoons C + D$.Species$A$$B$$C$$D$Initial moles$1$$1$$0$$0$Moles at equilibrium$(1-x)$$(1-x)$$x$$x$Given that at equilibrium,the number of moles of $C$ formed is $x = 0.5 \ mol$.Therefore,the moles of $A$ and $B$ remaining are $(1 - 0.5) = 0.5 \ mol$ each,and the moles of $D$ formed are $0.5 \ mol$.Since the volume of the flask is $1 \ L$,the concentrations are equal to the number of moles.$K_C = \frac{[C][D]}{[A][B]} = \frac{0.5 \times 0.5}{0.5 \times 0.5} = 1$.

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

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When one mole of $A$ and one mole of $B$ were heated in a one-litre flask at $T \ K$,$0.5 \ mole$ of $C$ was formed at equilibrium for the reaction $A + B \rightleftharpoons C + D$. The equilibrium constant,$K_C$,is:

TS EAMCET 2015 All TS EAMCET

A
$0.25$
B
$0.5$
C
$1$
D
$2$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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At $500 \ K$,for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the $K_p$ is $0.036 \ atm^{-2}$. What is its $K_C$ in $L^2 \ mol^{-2}$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

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In which of the following reactions is $K_p = K_c$?

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For the reaction,$H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,which of the following relations is correct?

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For the reaction $A + B \rightleftharpoons C + D$,the initial concentrations of $A$ and $B$ are equal. If the equilibrium concentration of $D$ is twice the equilibrium concentration of $A$,then the equilibrium constant $K_c$ is:

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For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Given $R = 0.0831 \, kJ/(mol \cdot K)$,when $K_p$ and $K_c$ are compared at $184 \, ^\circ C$,it is found that:

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When one mole of $A$ and one mole of $B$ were heated in a one-litre flask at $T \ K$,$0.5 \ mole$ of $C$ was formed at equilibrium for the reaction $A + B \rightleftharpoons C + D$. The equilibrium constant,$K_C$,is:

Similar Questions

At $500 \ K$,for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the $K_p$ is $0.036 \ atm^{-2}$. What is its $K_C$ in $L^2 \ mol^{-2}$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

In which of the following reactions is $K_p = K_c$?

For the reaction,$H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,which of the following relations is correct?

For the reaction $A + B \rightleftharpoons C + D$,the initial concentrations of $A$ and $B$ are equal. If the equilibrium concentration of $D$ is twice the equilibrium concentration of $A$,then the equilibrium constant $K_c$ is:

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Given $R = 0.0831 \, kJ/(mol \cdot K)$,when $K_p$ and $K_c$ are compared at $184 \, ^\circ C$,it is found that:

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