(B) The Van't Hoff equation relates the equilibrium constant $(K)$ to temperature $(T)$: $\ln(\frac{K_2}{K_1}) = \frac{-\Delta H}{R} (\frac{1}{T_2} -

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(B) The Van't Hoff equation relates the equilibrium constant $(K)$ to temperature $(T)$: $\ln(\frac{K_2}{K_1}) = \frac{-\Delta H}{R} (\frac{1}{T_2} - \frac{1}{T_1})$.Given $T_2 > T_1$ $(1000 \ K > 298 \ K)$ and $K_2 Since $(\frac{1}{T_2} - \frac{1}{T_1})$ is negative,the equation implies that $\Delta H$ must be negative for the equality to hold.Therefore,the reaction is exothermic,and $\Delta H < 0$.

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

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The equilibrium constant of a reaction at $298 \ K$ is $5 \times 10^{-3}$ and at $1000 \ K$ is $2 \times 10^{-5}$. What is the sign of $\Delta H$ for the reaction?

A
$\Delta H = 0$
B
$\Delta H$ is negative
C
$\Delta H$ is positive
D
None of these

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6-1.Equilibrium (Chemical Equilibrium)

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

For the equilibrium $ \text{Liquid} \rightleftharpoons \text{Vapour} $,which of the following expressions is correct?

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$56 \, g$ of nitrogen and $8 \, g$ of hydrogen gas are heated in a closed vessel. At equilibrium,$34 \, g$ of ammonia are present. The equilibrium number of moles of nitrogen,hydrogen,and ammonia are respectively:

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For the reaction $N_2 + O_2 \rightleftharpoons 2NO$,the equilibrium concentrations of $N_2$,$O_2$,and $NO$ are $0.25 \ mol/L$,$0.05 \ mol/L$,and $1.0 \ mol/L$ respectively. What are the initial concentrations of $N_2$ and $O_2$?

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$N_2O_{4(g)}$ at $300 \ K$ is kept in a closed container under $1 \ atm$. At equilibrium,$20\%$ of $N_2O_{4(g)}$ is converted to $NO_{2(g)}$.
$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
Hence,the resultant pressure is: (in $atm$)

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For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,at equilibrium,the mole fraction of $PCl_5$ is $0.4$ and the mole fraction of $Cl_2$ is $0.3$. What will be the mole fraction of $PCl_3$?

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The equilibrium constant of a reaction at $298 \ K$ is $5 \times 10^{-3}$ and at $1000 \ K$ is $2 \times 10^{-5}$. What is the sign of $\Delta H$ for the reaction?

Similar Questions

For the equilibrium $ \text{Liquid} \rightleftharpoons \text{Vapour} $,which of the following expressions is correct?

$56 \, g$ of nitrogen and $8 \, g$ of hydrogen gas are heated in a closed vessel. At equilibrium,$34 \, g$ of ammonia are present. The equilibrium number of moles of nitrogen,hydrogen,and ammonia are respectively:

For the reaction $N_2 + O_2 \rightleftharpoons 2NO$,the equilibrium concentrations of $N_2$,$O_2$,and $NO$ are $0.25 \ mol/L$,$0.05 \ mol/L$,and $1.0 \ mol/L$ respectively. What are the initial concentrations of $N_2$ and $O_2$?

$N_2O_{4(g)}$ at $300 \ K$ is kept in a closed container under $1 \ atm$. At equilibrium,$20\%$ of $N_2O_{4(g)}$ is converted to $NO_{2(g)}$.$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$Hence,the resultant pressure is: (in $atm$)

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,at equilibrium,the mole fraction of $PCl_5$ is $0.4$ and the mole fraction of $Cl_2$ is $0.3$. What will be the mole fraction of $PCl_3$?

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$N_2O_{4(g)}$ at $300 \ K$ is kept in a closed container under $1 \ atm$. At equilibrium,$20\%$ of $N_2O_{4(g)}$ is converted to $NO_{2(g)}$.
$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
Hence,the resultant pressure is: (in $atm$)