(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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Some solid $NH_4HS$ is placed in a flask containing $0.5 \ atm$ of $NH_3$. What would be the partial pressures of $NH_3$ and $H_2S$ when equilibrium is reached for the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$,given $K_p = 0.11$?

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For the reaction ${N_2}_{(g)} + 3{H_2}_{(g)} \rightleftharpoons 2{NH_3}_{(g)}$,the equilibrium constant ${K_P}$ is $5.8 \times 10^5$ at $298 \ K$. Calculate the value of the equilibrium constant ${K_C}$ (in $mol^{-2} \ L^2$) at the same temperature.

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$A_{(g)} + 3B_{(g)} \rightleftharpoons 4C_{(g)}$. The starting concentrations of $A$ and $B$ are equal. At equilibrium,the concentrations of $A$ and $C$ are the same. The value of $K_c$ is:

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For the reaction $CO_{(g)} + Cl_{2_{(g)}} \rightleftharpoons COCl_{2_{(g)}}$,the value of $\frac{K_p}{K_c}$ is .........

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What is the unit of $K_p$ for the reaction?
$CS_{2(g)} + 4H_{2(g)} \to CH_{4(g)} + 2H_2S_{(g)}$

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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:

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Some solid $NH_4HS$ is placed in a flask containing $0.5 \ atm$ of $NH_3$. What would be the partial pressures of $NH_3$ and $H_2S$ when equilibrium is reached for the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3_{(g)}} + H_2S_{(g)}$,given $K_p = 0.11$?

For the reaction ${N_2}_{(g)} + 3{H_2}_{(g)} \rightleftharpoons 2{NH_3}_{(g)}$,the equilibrium constant ${K_P}$ is $5.8 \times 10^5$ at $298 \ K$. Calculate the value of the equilibrium constant ${K_C}$ (in $mol^{-2} \ L^2$) at the same temperature.

$A_{(g)} + 3B_{(g)} \rightleftharpoons 4C_{(g)}$. The starting concentrations of $A$ and $B$ are equal. At equilibrium,the concentrations of $A$ and $C$ are the same. The value of $K_c$ is:

For the reaction $CO_{(g)} + Cl_{2_{(g)}} \rightleftharpoons COCl_{2_{(g)}}$,the value of $\frac{K_p}{K_c}$ is .........

What is the unit of $K_p$ for the reaction?$CS_{2(g)} + 4H_{2(g)} \to CH_{4(g)} + 2H_2S_{(g)}$

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What is the unit of $K_p$ for the reaction?
$CS_{2(g)} + 4H_{2(g)} \to CH_{4(g)} + 2H_2S_{(g)}$