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Q.

At 700K, the equilibrium constant K_P for the reaction 2SO_3(g) $⇌$ 2SO_2(g) + O_2(g) is 1.80 × 10^–3 , (R = 8.314 JK^–1 mole^–1). The numerical value in moles per lit of K_C for this reaction at the same temperature will be

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a

3.09 \times {10^{ - 7}}\,mol/L

b

8.18 \times {10^{ - 9}}\,mol/L

c

5.07 \times {10^{ - 8}}\,mol/L

d

9.24 \times {10^{ - 10}}\,mol/L

answer is A.

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Detailed Solution

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$\large 2S{O_3}\left( g \right) \rightleftharpoons 2S{O_2}\left( g \right) + {O_2}\left( g \right)$

$\large {K_P} = {K_C}{\left( {RT} \right)^{\Delta ng}}$

$\large \Rightarrow 1.8 \times {10^{ - 3}} = {K_C} \times {\left( {8.314 \times 700} \right)^1}$

$\large {K_C} = 0.0309 \times {10^{ - 5}} = 3.09 \times {10^{ - 7}}$

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At 700K, the equilibrium constant KP for the reaction 2SO3(g)⇌2SO2(g) + O2(g) is 1.80 × 10–3 , (R = 8.314 JK–1 mole–1). The numerical value in moles per lit of KC for this reaction at the same temperature will be