229241 $K_{c}$ for the reaction $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NO}(\mathrm{g})$
at $300 \mathrm{~K}$ is $4 \times 10^{-6}$. $\mathrm{K}_{\mathrm{p}}$ for the above reaction
$\text { will be }\left(R=2 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$

229242 A sample of $\mathrm{HI}(\mathrm{g})$ is placed in a flask at a pressure of $0.2 \mathrm{~atm}$. At equilibrium, partial pressure of $\mathrm{HI}(\mathrm{g})$ is $0.04 \mathrm{~atm}$. What is $K_{p}$ for the given equilibrium?
2HI $(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$

229243 What will be the expression of $K_{p}$ for the given reaction if the total pressure inside the vessel is $P$ and degree of dissociation of the reactant is a ? The reaction : $\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$

229245 The relationship between $K_{p}$ and $K_{c}$ is $K_{p}=K_{c}$ $(R T)^{\Delta n}$. What would be the value of $\Delta n$ for the reaction
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{HCl}(\mathrm{g})$ ?

229241 $K_{c}$ for the reaction $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NO}(\mathrm{g})$
at $300 \mathrm{~K}$ is $4 \times 10^{-6}$. $\mathrm{K}_{\mathrm{p}}$ for the above reaction
$\text { will be }\left(R=2 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$

229242 A sample of $\mathrm{HI}(\mathrm{g})$ is placed in a flask at a pressure of $0.2 \mathrm{~atm}$. At equilibrium, partial pressure of $\mathrm{HI}(\mathrm{g})$ is $0.04 \mathrm{~atm}$. What is $K_{p}$ for the given equilibrium?
2HI $(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$

229243 What will be the expression of $K_{p}$ for the given reaction if the total pressure inside the vessel is $P$ and degree of dissociation of the reactant is a ? The reaction : $\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$

229245 The relationship between $K_{p}$ and $K_{c}$ is $K_{p}=K_{c}$ $(R T)^{\Delta n}$. What would be the value of $\Delta n$ for the reaction
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{HCl}(\mathrm{g})$ ?

229241 $K_{c}$ for the reaction $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NO}(\mathrm{g})$
at $300 \mathrm{~K}$ is $4 \times 10^{-6}$. $\mathrm{K}_{\mathrm{p}}$ for the above reaction
$\text { will be }\left(R=2 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$

229242 A sample of $\mathrm{HI}(\mathrm{g})$ is placed in a flask at a pressure of $0.2 \mathrm{~atm}$. At equilibrium, partial pressure of $\mathrm{HI}(\mathrm{g})$ is $0.04 \mathrm{~atm}$. What is $K_{p}$ for the given equilibrium?
2HI $(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$

229243 What will be the expression of $K_{p}$ for the given reaction if the total pressure inside the vessel is $P$ and degree of dissociation of the reactant is a ? The reaction : $\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$

229245 The relationship between $K_{p}$ and $K_{c}$ is $K_{p}=K_{c}$ $(R T)^{\Delta n}$. What would be the value of $\Delta n$ for the reaction
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{HCl}(\mathrm{g})$ ?

229241 $K_{c}$ for the reaction $\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NO}(\mathrm{g})$
at $300 \mathrm{~K}$ is $4 \times 10^{-6}$. $\mathrm{K}_{\mathrm{p}}$ for the above reaction
$\text { will be }\left(R=2 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$

229242 A sample of $\mathrm{HI}(\mathrm{g})$ is placed in a flask at a pressure of $0.2 \mathrm{~atm}$. At equilibrium, partial pressure of $\mathrm{HI}(\mathrm{g})$ is $0.04 \mathrm{~atm}$. What is $K_{p}$ for the given equilibrium?
2HI $(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$

229243 What will be the expression of $K_{p}$ for the given reaction if the total pressure inside the vessel is $P$ and degree of dissociation of the reactant is a ? The reaction : $\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$

229245 The relationship between $K_{p}$ and $K_{c}$ is $K_{p}=K_{c}$ $(R T)^{\Delta n}$. What would be the value of $\Delta n$ for the reaction
$\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{HCl}(\mathrm{g})$ ?