229218
In the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$, relation between $K_{p}$ and $K_{c}$ is
Given the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$ $\therefore \Delta \mathrm{n}_{\mathrm{g}}=$ No. of mole of gaseous product - no. of moles of gaseous reactant $\begin{array}{ll} & =2-(1+1) \\ & \Delta \mathrm{n}_{\mathrm{g}}=0 \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{\Delta \mathrm{n}_{\mathrm{g}}} \\ & \mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})^{0} \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \end{array}$
[J and K CET-2008
Chemical Equilibrium
229219
For the reaction $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HI}(\mathrm{g})$, the equilibrium constant $K_{p}$ changes with
1 total pressure
2 catalyst
3 the amount $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$
4 temperature
Explanation:
The equilibrium constant $\mathrm{K}_{\mathrm{p}}$ will change with temperature. For the reaction- $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{HI}(\mathrm{g})$. Catalyst does not alter the state of equilibrium. Equilibrium constant depends only upon temperature. The relation of $\mathrm{K}$ with temperature can be shown as- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left[\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right]$
J and K CET-(2011)
Chemical Equilibrium
229220
In which of the following equilibrium $K_{c}$ and $K_{p}$ are not equal?
1 $2 \mathrm{C}$ (s) $+\mathrm{O}_{2}$ (g) $\rightleftharpoons 2 \mathrm{CO}_{2}$ (g)
229218
In the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$, relation between $K_{p}$ and $K_{c}$ is
Given the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$ $\therefore \Delta \mathrm{n}_{\mathrm{g}}=$ No. of mole of gaseous product - no. of moles of gaseous reactant $\begin{array}{ll} & =2-(1+1) \\ & \Delta \mathrm{n}_{\mathrm{g}}=0 \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{\Delta \mathrm{n}_{\mathrm{g}}} \\ & \mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})^{0} \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \end{array}$
[J and K CET-2008
Chemical Equilibrium
229219
For the reaction $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HI}(\mathrm{g})$, the equilibrium constant $K_{p}$ changes with
1 total pressure
2 catalyst
3 the amount $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$
4 temperature
Explanation:
The equilibrium constant $\mathrm{K}_{\mathrm{p}}$ will change with temperature. For the reaction- $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{HI}(\mathrm{g})$. Catalyst does not alter the state of equilibrium. Equilibrium constant depends only upon temperature. The relation of $\mathrm{K}$ with temperature can be shown as- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left[\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right]$
J and K CET-(2011)
Chemical Equilibrium
229220
In which of the following equilibrium $K_{c}$ and $K_{p}$ are not equal?
1 $2 \mathrm{C}$ (s) $+\mathrm{O}_{2}$ (g) $\rightleftharpoons 2 \mathrm{CO}_{2}$ (g)
229218
In the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$, relation between $K_{p}$ and $K_{c}$ is
Given the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$ $\therefore \Delta \mathrm{n}_{\mathrm{g}}=$ No. of mole of gaseous product - no. of moles of gaseous reactant $\begin{array}{ll} & =2-(1+1) \\ & \Delta \mathrm{n}_{\mathrm{g}}=0 \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{\Delta \mathrm{n}_{\mathrm{g}}} \\ & \mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})^{0} \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \end{array}$
[J and K CET-2008
Chemical Equilibrium
229219
For the reaction $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HI}(\mathrm{g})$, the equilibrium constant $K_{p}$ changes with
1 total pressure
2 catalyst
3 the amount $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$
4 temperature
Explanation:
The equilibrium constant $\mathrm{K}_{\mathrm{p}}$ will change with temperature. For the reaction- $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{HI}(\mathrm{g})$. Catalyst does not alter the state of equilibrium. Equilibrium constant depends only upon temperature. The relation of $\mathrm{K}$ with temperature can be shown as- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left[\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right]$
J and K CET-(2011)
Chemical Equilibrium
229220
In which of the following equilibrium $K_{c}$ and $K_{p}$ are not equal?
1 $2 \mathrm{C}$ (s) $+\mathrm{O}_{2}$ (g) $\rightleftharpoons 2 \mathrm{CO}_{2}$ (g)
229218
In the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$, relation between $K_{p}$ and $K_{c}$ is
Given the reaction, $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g})$ $\therefore \Delta \mathrm{n}_{\mathrm{g}}=$ No. of mole of gaseous product - no. of moles of gaseous reactant $\begin{array}{ll} & =2-(1+1) \\ & \Delta \mathrm{n}_{\mathrm{g}}=0 \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}}(\mathrm{RT})^{\Delta \mathrm{n}_{\mathrm{g}}} \\ & \mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \times(\mathrm{RT})^{0} \\ & \mathrm{~K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{c}} \end{array}$
[J and K CET-2008
Chemical Equilibrium
229219
For the reaction $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HI}(\mathrm{g})$, the equilibrium constant $K_{p}$ changes with
1 total pressure
2 catalyst
3 the amount $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$
4 temperature
Explanation:
The equilibrium constant $\mathrm{K}_{\mathrm{p}}$ will change with temperature. For the reaction- $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{HI}(\mathrm{g})$. Catalyst does not alter the state of equilibrium. Equilibrium constant depends only upon temperature. The relation of $\mathrm{K}$ with temperature can be shown as- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left[\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right]$
J and K CET-(2011)
Chemical Equilibrium
229220
In which of the following equilibrium $K_{c}$ and $K_{p}$ are not equal?
1 $2 \mathrm{C}$ (s) $+\mathrm{O}_{2}$ (g) $\rightleftharpoons 2 \mathrm{CO}_{2}$ (g)