(A) The reaction is: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$Initial moles: $N_2 = 2, H_2 = 6, NH_3 = 0$At equilibrium: $N_2 = (2 - x), H_

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(A) The reaction is: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$Initial moles: $N_2 = 2, H_2 = 6, NH_3 = 0$At equilibrium: $N_2 = (2 - x), H_2 = (6 - 3x), NH_3 = 2x$Given that $50\%$ of $N_2$ is converted,so $x = 2 \times 0.5 = 1 \ mol$.Equilibrium concentrations (in $1 \ L$ volume): $[N_2] = 2 - 1 = 1 \ M$,$[H_2] = 6 - 3(1) = 3 \ M$,$[NH_3] = 2(1) = 2 \ M$.$K_c = \frac{[NH_3]^2}{[N_2][H_2]^3} = \frac{(2)^2}{(1)(3)^3} = \frac{4}{27}$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Medium

In a closed vessel of $1 \ L$ capacity,$2 \ mol$ of $N_2$ and $6 \ mol$ of $H_2$ are mixed. If at equilibrium $50\% \ N_2$ is converted into $NH_3$,then the value of $K_c$ for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ will be:

A
$\frac{4}{27}$
B
$\frac{27}{4}$
C
$\frac{1}{27}$
D
$24$

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6-1.Equilibrium (Chemical Equilibrium)

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

For the reaction $A + B \rightleftharpoons C + D$ at $250^\circ C$ in a $1 \ L$ vessel,the initial concentration of $A$ is $3$ and $B$ is $n$. If the equilibrium concentration of $C$ is equal to the equilibrium concentration of $B$,what is the equilibrium concentration of $D$?

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At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.
$(i)$ Find $K_p$.
$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?

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At $1000 \ K$ in a $0.654 \ L$ vessel,$CaCO_{3(s)}$ is taken. For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the equilibrium constant $K_p$ is $3.9 \times 10^{-2} \ bar$. Find the weight of $CaO$ produced at equilibrium. $(Ca=40, C=12, O=16)$

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$2SO_2 + O_2 \to$ product. If the pressure of the reaction increases $3$ times, then the rate will be (in $times$)?

Easy

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For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,what is the relationship between $\Delta H$ and $\Delta E$?

MediumAIPMT 2002

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In a closed vessel of $1 \ L$ capacity,$2 \ mol$ of $N_2$ and $6 \ mol$ of $H_2$ are mixed. If at equilibrium $50\% \ N_2$ is converted into $NH_3$,then the value of $K_c$ for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ will be:

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For the reaction $A + B \rightleftharpoons C + D$ at $250^\circ C$ in a $1 \ L$ vessel,the initial concentration of $A$ is $3$ and $B$ is $n$. If the equilibrium concentration of $C$ is equal to the equilibrium concentration of $B$,what is the equilibrium concentration of $D$?

At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.$(i)$ Find $K_p$.$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?

At $1000 \ K$ in a $0.654 \ L$ vessel,$CaCO_{3(s)}$ is taken. For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the equilibrium constant $K_p$ is $3.9 \times 10^{-2} \ bar$. Find the weight of $CaO$ produced at equilibrium. $(Ca=40, C=12, O=16)$

$2SO_2 + O_2 \to$ product. If the pressure of the reaction increases $3$ times, then the rate will be (in $times$)?

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,what is the relationship between $\Delta H$ and $\Delta E$?

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At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.
$(i)$ Find $K_p$.
$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?