Given the reaction between 2 gases represented by A2 and B2 to give the compound ABg- A2g-B2g- 2ABgAt equilibrium- the concentrationof A2-3-0-10-3Mof B2-4-2-10-3Mof AB-2-8-10-3MIf the reaction takes place in a sealed vessel at 527oC- then the value of Kc will be-

The correct option is B 0.62 The equilibrium reaction is as given below. A_2+B_2⇌ #160;2AB The expression for the equilibrium constant is as given b ...

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Standard XII

Chemistry

Introduction

Given the rea...

Question

Given the reaction between 2 gases represented by $A_{2}$ and $B_{2}$ to give the compound ${A B}_{(g)}$ .
$A_{2 (g)} + B_{2 (g)} ⇌ 2 {A B}_{(g)}$
At equilibrium, the concentration
of $A_{2} = 3.0 \times 10^{- 3} M$
of $B_{2} = 4.2 \times 10^{- 3} M$
of $A B = 2.8 \times 10^{- 3} M$
If the reaction takes place in a sealed vessel at $527^{o} C$ , then the value of $K_{c}$ will be:

1.9

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0.62

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4.5

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2.0

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Solution

The correct option is B $0.62$
The equilibrium reaction is as given below.
$A_{2} + B_{2} ⇌ 2 A B$

The expression for the equilibrium constant is as given below.

$K_{c} = \frac{{[A B]}^{2}}{[A_{2}] [B_{2}]}$

Substitute values in the above expression.

$K_{c} = \frac{2.8 \times 2.8 \times 10^{- 6}}{3 \times 10^{- 3} \times 4.2 \times 10^{- 3}} = 0.62$ .

Hence, the value of the equilibrium constant is 0.62.

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Given the reaction between 2 gases represented by A2 and B2 to give the compound AB(g).A2(g)+B2(g)⇌2AB(g)At equilibrium, the concentrationof A2=3.0×10−3Mof B2=4.2×10−3Mof AB=2.8×10−3MIf the reaction takes place in a sealed vessel at 527oC, then the value of Kc will be: