(C) Given reactions:$(i) \ 2 A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)} ; K_1 = 16$$(ii) \ 2 B_{(g)} + C_{(g)} \rightleftharpoons 2 D_{(g)} ; K_2 =

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(C) Given reactions:$(i) \ 2 A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)} ; K_1 = 16$$(ii) \ 2 B_{(g)} + C_{(g)} \rightleftharpoons 2 D_{(g)} ; K_2 = 25$We need the equilibrium constant $(K_3)$ for:$(iii) \ A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons D_{(g)}$From $(i)$,$K_1 = \frac{[B][C]}{[A]^2} = 16$.From $(ii)$,$K_2 = \frac{[D]^2}{[C][B]^2} = 25$.Multiplying $(i)$ and $(ii)$:$K_1 \times K_2 = \frac{[B][C]}{[A]^2} \times \frac{[D]^2}{[C][B]^2} = \frac{[D]^2}{[A]^2 [B]} = 16 \times 25 = 400$.Taking the square root of the expression:$\sqrt{\frac{[D]^2}{[A]^2 [B]}} = \frac{[D]}{[A][B]^{1/2}} = \sqrt{400} = 20$.Thus,$K_3 = 20$.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Law of equilibrium and Equilibrium constant

Medium

At $T \ K$,the equilibrium constants for the following two reactions are given below:
$2 A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)} ; K_1 = 16$
$2 B_{(g)} + C_{(g)} \rightleftharpoons 2 D_{(g)} ; K_2 = 25$
What is the value of equilibrium constant $(K)$ for the reaction given below at $T \ K$?
$A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons D_{(g)}$

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A
$100$
B
$50$
C
$20$
D
$75$

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1 Equilibrium: Chemical Equilibrium

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Law of equilibrium and Equilibrium constant

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Steam reacts with iron at high temperature to give hydrogen gas and $Fe_3O_{4(s)}$. The correct expression for the equilibrium constant is

$A$ reaction is $A + B \rightleftharpoons C + D$. Initially,we start with equal concentrations of $A$ and $B$. At equilibrium,the number of moles of $C$ is two times that of $A$. What is the equilibrium constant $(K_c)$ of the reaction?

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$N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$

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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
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