In which of the following equilibrium reactio | vedclass

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(A) According to Le Chatelier’s principle,when the total pressure of a system at equilibrium is increased,the equilibrium shifts in the direction that

Vedclass · Accepted Answer

$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$

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(A) According to Le Chatelier’s principle,when the total pressure of a system at equilibrium is increased,the equilibrium shifts in the direction that produces a smaller number of moles of gaseous species to counteract the pressure increase.For the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$,the number of moles of gaseous reactants is $1 + 3 = 4$,and the number of moles of gaseous products is $2$.Since the product side has fewer moles $(2 For options $B$ and $C$,the number of moles of gaseous reactants equals the number of moles of gaseous products $(2 = 2)$,so pressure change has no effect.For option $D$,the product side has more moles $(2 > 1)$,so increasing pressure shifts the equilibrium to the left.

In which of the following equilibrium reactions,the equilibrium would shift to the right,if total pressure is increased?

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