229063 Assertion: At equilibrium, $\Delta \mathrm{G}=0$.
Reason: At equilibrium, $\Delta \mathrm{G}^{\mathrm{o}}=\mathrm{RT} \log \mathrm{K}_{\mathrm{c}}$.

229064 The value of $\log _{10} K$ for the reaction $A \rightleftharpoons B$ is
(Given : $\Delta_{\mathrm{f}} \mathrm{H}^{0}(298 \mathrm{~K})=-54.07 \mathrm{kJmol}^{-1}$
$\begin{aligned}
& \Delta_{\mathrm{r}} \mathrm{S}^{0}=10 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \\
& \left.\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)
\end{aligned}$

229065 The dissociation energy of $\mathrm{CH}_{4}$ and $\mathrm{C}_{6} \mathrm{H}_{6}$ to convert them into gaseous atom are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

229067 $\Delta_{r} G^{\circ}$ for the conversion of $O_{2}$ to ozone, $\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{O}_{3}(\mathrm{~g})$ at $298 \mathrm{~K}$ is
( $K_{\mathrm{p}}$ for this conversion is $1 \times 10^{-29}$ )

229069 If the activation energy for the forward reaction is $150 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and that of the reverse reaction is $260 \mathrm{~kJ} \mathrm{~mol}^{-1}$. What is the enthalpy change for the reaction?

229063 Assertion: At equilibrium, $\Delta \mathrm{G}=0$.
Reason: At equilibrium, $\Delta \mathrm{G}^{\mathrm{o}}=\mathrm{RT} \log \mathrm{K}_{\mathrm{c}}$.

229064 The value of $\log _{10} K$ for the reaction $A \rightleftharpoons B$ is
(Given : $\Delta_{\mathrm{f}} \mathrm{H}^{0}(298 \mathrm{~K})=-54.07 \mathrm{kJmol}^{-1}$
$\begin{aligned}
& \Delta_{\mathrm{r}} \mathrm{S}^{0}=10 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \\
& \left.\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)
\end{aligned}$

229065 The dissociation energy of $\mathrm{CH}_{4}$ and $\mathrm{C}_{6} \mathrm{H}_{6}$ to convert them into gaseous atom are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

229067 $\Delta_{r} G^{\circ}$ for the conversion of $O_{2}$ to ozone, $\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{O}_{3}(\mathrm{~g})$ at $298 \mathrm{~K}$ is
( $K_{\mathrm{p}}$ for this conversion is $1 \times 10^{-29}$ )

229069 If the activation energy for the forward reaction is $150 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and that of the reverse reaction is $260 \mathrm{~kJ} \mathrm{~mol}^{-1}$. What is the enthalpy change for the reaction?

229063 Assertion: At equilibrium, $\Delta \mathrm{G}=0$.
Reason: At equilibrium, $\Delta \mathrm{G}^{\mathrm{o}}=\mathrm{RT} \log \mathrm{K}_{\mathrm{c}}$.

229064 The value of $\log _{10} K$ for the reaction $A \rightleftharpoons B$ is
(Given : $\Delta_{\mathrm{f}} \mathrm{H}^{0}(298 \mathrm{~K})=-54.07 \mathrm{kJmol}^{-1}$
$\begin{aligned}
& \Delta_{\mathrm{r}} \mathrm{S}^{0}=10 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \\
& \left.\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)
\end{aligned}$

229065 The dissociation energy of $\mathrm{CH}_{4}$ and $\mathrm{C}_{6} \mathrm{H}_{6}$ to convert them into gaseous atom are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

229067 $\Delta_{r} G^{\circ}$ for the conversion of $O_{2}$ to ozone, $\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{O}_{3}(\mathrm{~g})$ at $298 \mathrm{~K}$ is
( $K_{\mathrm{p}}$ for this conversion is $1 \times 10^{-29}$ )

229069 If the activation energy for the forward reaction is $150 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and that of the reverse reaction is $260 \mathrm{~kJ} \mathrm{~mol}^{-1}$. What is the enthalpy change for the reaction?

229063 Assertion: At equilibrium, $\Delta \mathrm{G}=0$.
Reason: At equilibrium, $\Delta \mathrm{G}^{\mathrm{o}}=\mathrm{RT} \log \mathrm{K}_{\mathrm{c}}$.

229064 The value of $\log _{10} K$ for the reaction $A \rightleftharpoons B$ is
(Given : $\Delta_{\mathrm{f}} \mathrm{H}^{0}(298 \mathrm{~K})=-54.07 \mathrm{kJmol}^{-1}$
$\begin{aligned}
& \Delta_{\mathrm{r}} \mathrm{S}^{0}=10 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \\
& \left.\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)
\end{aligned}$

229065 The dissociation energy of $\mathrm{CH}_{4}$ and $\mathrm{C}_{6} \mathrm{H}_{6}$ to convert them into gaseous atom are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

229067 $\Delta_{r} G^{\circ}$ for the conversion of $O_{2}$ to ozone, $\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{O}_{3}(\mathrm{~g})$ at $298 \mathrm{~K}$ is
( $K_{\mathrm{p}}$ for this conversion is $1 \times 10^{-29}$ )

229069 If the activation energy for the forward reaction is $150 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and that of the reverse reaction is $260 \mathrm{~kJ} \mathrm{~mol}^{-1}$. What is the enthalpy change for the reaction?

229063 Assertion: At equilibrium, $\Delta \mathrm{G}=0$.
Reason: At equilibrium, $\Delta \mathrm{G}^{\mathrm{o}}=\mathrm{RT} \log \mathrm{K}_{\mathrm{c}}$.

229064 The value of $\log _{10} K$ for the reaction $A \rightleftharpoons B$ is
(Given : $\Delta_{\mathrm{f}} \mathrm{H}^{0}(298 \mathrm{~K})=-54.07 \mathrm{kJmol}^{-1}$
$\begin{aligned}
& \Delta_{\mathrm{r}} \mathrm{S}^{0}=10 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \\
& \left.\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)
\end{aligned}$

229065 The dissociation energy of $\mathrm{CH}_{4}$ and $\mathrm{C}_{6} \mathrm{H}_{6}$ to convert them into gaseous atom are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

229067 $\Delta_{r} G^{\circ}$ for the conversion of $O_{2}$ to ozone, $\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{O}_{3}(\mathrm{~g})$ at $298 \mathrm{~K}$ is
( $K_{\mathrm{p}}$ for this conversion is $1 \times 10^{-29}$ )

229069 If the activation energy for the forward reaction is $150 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and that of the reverse reaction is $260 \mathrm{~kJ} \mathrm{~mol}^{-1}$. What is the enthalpy change for the reaction?