For the reaction at equilibrium N_{2(g)} + 3H | vedclass

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(A) When an inert gas is added to a gaseous reaction at constant pressure,the total volume of the system increases.According to the ideal gas law,$PV

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Concentration of $N_2$ increases

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(A) When an inert gas is added to a gaseous reaction at constant pressure,the total volume of the system increases.According to the ideal gas law,$PV = nRT$,if $P$ and $T$ are constant,an increase in the total number of moles $(n)$ due to the addition of an inert gas leads to an increase in volume $(V)$.Since concentration is defined as $C = n/V$,an increase in $V$ results in a decrease in the concentration of all gaseous reactants and products.For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the reaction quotient $Q_c$ is given by $Q_c = [NH_3]^2 / ([N_2][H_2]^3)$.As the volume increases,the concentration of each species decreases. Since the denominator has a higher power $(1+3=4)$ than the numerator $(2)$,the value of $Q_c$ increases,making $Q_c > K_c$.This shift causes the equilibrium to move in the direction of fewer moles of gas (the backward direction in this case) to counteract the change.Therefore,the concentration of $N_2$ and $H_2$ will increase relative to their values immediately after the volume expansion,and the concentration of $NH_3$ will decrease.Option $A$ is incorrect because the concentration of $N_2$ decreases due to volume expansion,and it does not increase back to its original value.

For the reaction at equilibrium
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
On addition of an inert gas at constant pressure and constant temperature,which of the following changes is $NOT$ observed?

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For the reaction at equilibrium $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$On addition of an inert gas at constant pressure and constant temperature,which of the following changes is $NOT$ observed?