(A) The relationship between equilibrium constants at two different temperatures is given by the van't Hoff equation: $\log \frac{K'_p}{K_p} = -\frac{

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(A) The relationship between equilibrium constants at two different temperatures is given by the van't Hoff equation: $\log \frac{K'_p}{K_p} = -\frac{\Delta H}{2.303 R} \left[ \frac{1}{T_2} - \frac{1}{T_1} \right]$.For an exothermic reaction,the enthalpy change $\Delta H$ is negative $(\Delta H Given that $T_2 > T_1$,the term $\left( \frac{1}{T_2} - \frac{1}{T_1} \right)$ is negative.Substituting these into the equation: $\log \frac{K'_p}{K_p} = -\frac{(-ve)}{2.303 R} \times (-ve) = -ve$.Since $\log \frac{K'_p}{K_p} K'_p$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

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For a given exothermic reaction,$K_p$ and $K'_p$ are the equilibrium constants at temperatures $T_1$ and $T_2,$ respectively. Assuming that the heat of reaction is constant in the temperature range between $T_1$ and $T_2,$ where $T_2 > T_1,$ it is readily observed that:

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A
$K_p > K'_p$
B
$K_p < K'_p$
C
$K_p = K'_p$
D
$K_p = \frac{1}{K'_p}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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For the reaction $2AB_{(g)} \rightleftharpoons 2A_{(g)} + B_{2(g)}$,$AB$ dissociates. If the initial pressure of $AB$ is $500 \, mm$ and the total pressure at equilibrium is $625 \, mm$,calculate $K_p$ for the reaction. Assume constant volume.

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$(i)$ $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$ at $298 \ K$ has $\Delta G^{\Theta} = -16.5 \ kJ \ mol^{-1}$. Find $K_p$.
$(ii)$ At $298 \ K$,for $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,calculate $K_p$ and $\Delta G^{\Theta}$.

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For the gaseous reaction $aA + bB \rightleftharpoons cC + dD$,the relation between $K_p$ and $K_c$ is:

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For which of the following reactions will the value of $\Delta n = \sum n_p - \sum n_r$ be positive? $(1)$ $C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$ $(2)$ $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ $(3)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

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For a given exothermic reaction,$K_p$ and $K'_p$ are the equilibrium constants at temperatures $T_1$ and $T_2,$ respectively. Assuming that the heat of reaction is constant in the temperature range between $T_1$ and $T_2,$ where $T_2 > T_1,$ it is readily observed that:

Similar Questions

For the reaction $2AB_{(g)} \rightleftharpoons 2A_{(g)} + B_{2(g)}$,$AB$ dissociates. If the initial pressure of $AB$ is $500 \, mm$ and the total pressure at equilibrium is $625 \, mm$,calculate $K_p$ for the reaction. Assume constant volume.

$(i)$ $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$ at $298 \ K$ has $\Delta G^{\Theta} = -16.5 \ kJ \ mol^{-1}$. Find $K_p$.$(ii)$ At $298 \ K$,for $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,calculate $K_p$ and $\Delta G^{\Theta}$.

For the gaseous reaction $aA + bB \rightleftharpoons cC + dD$,the relation between $K_p$ and $K_c$ is:

For which of the following reactions will the value of $\Delta n = \sum n_p - \sum n_r$ be positive? $(1)$ $C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$ $(2)$ $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ $(3)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

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$(i)$ $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$ at $298 \ K$ has $\Delta G^{\Theta} = -16.5 \ kJ \ mol^{-1}$. Find $K_p$.
$(ii)$ At $298 \ K$,for $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,calculate $K_p$ and $\Delta G^{\Theta}$.