Kp has the value of 10^-6 atm^3 and 10^-4 atm^3 at 298 K and 323 K respectively for the reacti

step 1 Here I can write the expression long Kp2 by Kp1 is equal to del H0 by R, 1 by T1 minus 1 by T2,

Kp has the value of 10^-6 atm^3 and 10^-4 atm^3 at 298 K...

$\mathrm{K}_{\mathrm{p}}$ has the value of $10^{-6} \mathrm{~atm}^3$ and $10^{-4} \mathrm{~atm}^3$ at 298 K and 323 K respectively for the reaction $\mathrm{CuSO}_4 \cdot 3 \mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightleftharpoons \mathrm{CuSO}_4(\mathrm{~s})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$ $\Delta_r \mathrm{H}^{\circ}$ for the reaction is: (a) $7.7 \mathrm{~kJ} / \mathrm{mol}$ (b) $-147.41 \mathrm{~kJ} / \mathrm{mol}$ (c) $147.41 \mathrm{~kJ} / \mathrm{mol}$ (d) None of these

$\mathrm{K}_{\mathrm{p}}$ has the value of $10^{-6} \mathrm{~atm}^3$ and $10^{-4} \mathrm{~atm}^3$ at 298 K and 323 K respectively for the reaction
$\mathrm{CuSO}_4 \cdot 3 \mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightleftharpoons \mathrm{CuSO}_4(\mathrm{~s})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$
$\Delta_r \mathrm{H}^{\circ}$ for the reaction is:
(a) $7.7 \mathrm{~kJ} / \mathrm{mol}$
(b) $-147.41 \mathrm{~kJ} / \mathrm{mol}$
(c) $147.41 \mathrm{~kJ} / \mathrm{mol}$
(d) None of these

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Key Concepts

Van't Hoff Equation

This equation relates the change in the equilibrium constant with temperature to the enthalpy change of the reaction. It is expressed as ln(K2/K1) = -?H°/R (1/T2 - 1/T1), where K1 and K2 are the equilibrium constants at temperatures T1 and T2, ?H° is the reaction enthalpy, and R is the gas constant. This relationship helps determine whether a reaction is endothermic or exothermic.

Equilibrium Constant (Kp)

This concept refers to the constant value that reflects the ratio of the partial pressures of the gaseous products to the gaseous reactants at equilibrium for a given chemical reaction and temperature. It is used to determine the position of equilibrium and to understand how the system responds to changes in conditions such as temperature or pressure.

Reaction Enthalpy (?H°)

This term represents the heat change during a chemical reaction at constant pressure. It indicates whether a reaction absorbs heat (endothermic) or releases heat (exothermic). Understanding the reaction enthalpy is crucial in predicting the temperature dependence of the equilibrium position and is directly linked with the equilibrium constant through the Van't Hoff equation.

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