229163
The chemical reaction of a gas phase is given below. $\mathbf{2 A}(\mathrm{g})+\mathbf{B}(\mathrm{g}) \rightleftharpoons \mathbf{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$ Which one of the following changes will affect the value of $K_{c}$ ?
1 Addition of inert gas
2 Increasing in temperature
3 Addition of reactants
4 Addition of catalyst
Explanation:
According to Vant Hoff equation- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left(\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right)$ If, $\Delta \mathrm{H}$ is positive then the reaction is endothermic then temperature increase also the $\mathrm{K}$ is increases. $\Delta \mathrm{H}$ is negative then the reaction is exothermic then temperature increases also $\mathrm{K}$ is decreases. $\mathrm{K}_{\mathrm{c}}$ is a function of temperature only.
Manipal-2016
Chemical Equilibrium
229165
Which one of the following is correct?
1 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ is independent of temperature
2 The value of $K_{c}$ is independent of initial concentrations of reactants and products
3 At equilibrium, the rate of the forward reaction is twice the rate of the backward reaction
4 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ for the reaction $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \text { is, } \frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]}$
Explanation:
(a) Equilibrium constant is temperature dependent having one unique value for a particular reaction represented by a balanced equation at a given temperature. (b) The value of equilibrium constant is independent of initial concentration of the reactants and products. (c) At equilibrium, the rate of forward reaction is equal to the rate of backward reaction. (d) For the equilibrium reaction- $\begin{array}{ll} & \mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \\ \therefore & \mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]^{4}} \end{array}$
TS-EAMCET-2016
Chemical Equilibrium
229169
Consider the following reaction $\mathrm{CaCO}_{3}(\mathrm{~s})$ $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ in closed container at equilibrium. What would be the effect of addition of $\mathrm{CaCO}_{3}$ on the equilibrium concentration of $\mathrm{CO}_{2}$ ?
229171
In a reaction, $A+B \rightleftharpoons C+D, 40 \%$ of $B$ has reacted at equilibrium, when 1 mole of $A$ was heated with 1 mole of $B$ in a $10 \mathrm{~L}$ closed vessel. The value of $K_{c}$ is
229180
The value of $\Delta H$ for the reaction $\mathbf{X}_{2}(\mathrm{~g})+\mathbf{4} \mathbf{Y}_{2}(\mathrm{~g}) \rightleftharpoons \mathbf{2} \mathbf{X Y}_{4}(\mathrm{~g})$ is less than zero formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at
1 high temperature and high pressure
2 low pressure and low temperature
3 high temperature and low pressure
4 high pressure and low temperature
Explanation:
The reaction is: $\begin{aligned} & \mathrm{X}_{2}(\mathrm{~g})+4 \mathrm{Y}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{XY}_{4}(\mathrm{~g}) \\ & \Delta \mathrm{n}_{\mathrm{g}}=-\mathrm{Ve} \end{aligned}$ And, $\quad \Delta \mathrm{H}=-\mathrm{Ve}$ So, formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at high pressure and low temperature.
229163
The chemical reaction of a gas phase is given below. $\mathbf{2 A}(\mathrm{g})+\mathbf{B}(\mathrm{g}) \rightleftharpoons \mathbf{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$ Which one of the following changes will affect the value of $K_{c}$ ?
1 Addition of inert gas
2 Increasing in temperature
3 Addition of reactants
4 Addition of catalyst
Explanation:
According to Vant Hoff equation- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left(\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right)$ If, $\Delta \mathrm{H}$ is positive then the reaction is endothermic then temperature increase also the $\mathrm{K}$ is increases. $\Delta \mathrm{H}$ is negative then the reaction is exothermic then temperature increases also $\mathrm{K}$ is decreases. $\mathrm{K}_{\mathrm{c}}$ is a function of temperature only.
Manipal-2016
Chemical Equilibrium
229165
Which one of the following is correct?
1 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ is independent of temperature
2 The value of $K_{c}$ is independent of initial concentrations of reactants and products
3 At equilibrium, the rate of the forward reaction is twice the rate of the backward reaction
4 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ for the reaction $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \text { is, } \frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]}$
Explanation:
(a) Equilibrium constant is temperature dependent having one unique value for a particular reaction represented by a balanced equation at a given temperature. (b) The value of equilibrium constant is independent of initial concentration of the reactants and products. (c) At equilibrium, the rate of forward reaction is equal to the rate of backward reaction. (d) For the equilibrium reaction- $\begin{array}{ll} & \mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \\ \therefore & \mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]^{4}} \end{array}$
TS-EAMCET-2016
Chemical Equilibrium
229169
Consider the following reaction $\mathrm{CaCO}_{3}(\mathrm{~s})$ $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ in closed container at equilibrium. What would be the effect of addition of $\mathrm{CaCO}_{3}$ on the equilibrium concentration of $\mathrm{CO}_{2}$ ?
229171
In a reaction, $A+B \rightleftharpoons C+D, 40 \%$ of $B$ has reacted at equilibrium, when 1 mole of $A$ was heated with 1 mole of $B$ in a $10 \mathrm{~L}$ closed vessel. The value of $K_{c}$ is
229180
The value of $\Delta H$ for the reaction $\mathbf{X}_{2}(\mathrm{~g})+\mathbf{4} \mathbf{Y}_{2}(\mathrm{~g}) \rightleftharpoons \mathbf{2} \mathbf{X Y}_{4}(\mathrm{~g})$ is less than zero formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at
1 high temperature and high pressure
2 low pressure and low temperature
3 high temperature and low pressure
4 high pressure and low temperature
Explanation:
The reaction is: $\begin{aligned} & \mathrm{X}_{2}(\mathrm{~g})+4 \mathrm{Y}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{XY}_{4}(\mathrm{~g}) \\ & \Delta \mathrm{n}_{\mathrm{g}}=-\mathrm{Ve} \end{aligned}$ And, $\quad \Delta \mathrm{H}=-\mathrm{Ve}$ So, formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at high pressure and low temperature.
229163
The chemical reaction of a gas phase is given below. $\mathbf{2 A}(\mathrm{g})+\mathbf{B}(\mathrm{g}) \rightleftharpoons \mathbf{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$ Which one of the following changes will affect the value of $K_{c}$ ?
1 Addition of inert gas
2 Increasing in temperature
3 Addition of reactants
4 Addition of catalyst
Explanation:
According to Vant Hoff equation- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left(\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right)$ If, $\Delta \mathrm{H}$ is positive then the reaction is endothermic then temperature increase also the $\mathrm{K}$ is increases. $\Delta \mathrm{H}$ is negative then the reaction is exothermic then temperature increases also $\mathrm{K}$ is decreases. $\mathrm{K}_{\mathrm{c}}$ is a function of temperature only.
Manipal-2016
Chemical Equilibrium
229165
Which one of the following is correct?
1 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ is independent of temperature
2 The value of $K_{c}$ is independent of initial concentrations of reactants and products
3 At equilibrium, the rate of the forward reaction is twice the rate of the backward reaction
4 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ for the reaction $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \text { is, } \frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]}$
Explanation:
(a) Equilibrium constant is temperature dependent having one unique value for a particular reaction represented by a balanced equation at a given temperature. (b) The value of equilibrium constant is independent of initial concentration of the reactants and products. (c) At equilibrium, the rate of forward reaction is equal to the rate of backward reaction. (d) For the equilibrium reaction- $\begin{array}{ll} & \mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \\ \therefore & \mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]^{4}} \end{array}$
TS-EAMCET-2016
Chemical Equilibrium
229169
Consider the following reaction $\mathrm{CaCO}_{3}(\mathrm{~s})$ $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ in closed container at equilibrium. What would be the effect of addition of $\mathrm{CaCO}_{3}$ on the equilibrium concentration of $\mathrm{CO}_{2}$ ?
229171
In a reaction, $A+B \rightleftharpoons C+D, 40 \%$ of $B$ has reacted at equilibrium, when 1 mole of $A$ was heated with 1 mole of $B$ in a $10 \mathrm{~L}$ closed vessel. The value of $K_{c}$ is
229180
The value of $\Delta H$ for the reaction $\mathbf{X}_{2}(\mathrm{~g})+\mathbf{4} \mathbf{Y}_{2}(\mathrm{~g}) \rightleftharpoons \mathbf{2} \mathbf{X Y}_{4}(\mathrm{~g})$ is less than zero formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at
1 high temperature and high pressure
2 low pressure and low temperature
3 high temperature and low pressure
4 high pressure and low temperature
Explanation:
The reaction is: $\begin{aligned} & \mathrm{X}_{2}(\mathrm{~g})+4 \mathrm{Y}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{XY}_{4}(\mathrm{~g}) \\ & \Delta \mathrm{n}_{\mathrm{g}}=-\mathrm{Ve} \end{aligned}$ And, $\quad \Delta \mathrm{H}=-\mathrm{Ve}$ So, formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at high pressure and low temperature.
229163
The chemical reaction of a gas phase is given below. $\mathbf{2 A}(\mathrm{g})+\mathbf{B}(\mathrm{g}) \rightleftharpoons \mathbf{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$ Which one of the following changes will affect the value of $K_{c}$ ?
1 Addition of inert gas
2 Increasing in temperature
3 Addition of reactants
4 Addition of catalyst
Explanation:
According to Vant Hoff equation- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left(\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right)$ If, $\Delta \mathrm{H}$ is positive then the reaction is endothermic then temperature increase also the $\mathrm{K}$ is increases. $\Delta \mathrm{H}$ is negative then the reaction is exothermic then temperature increases also $\mathrm{K}$ is decreases. $\mathrm{K}_{\mathrm{c}}$ is a function of temperature only.
Manipal-2016
Chemical Equilibrium
229165
Which one of the following is correct?
1 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ is independent of temperature
2 The value of $K_{c}$ is independent of initial concentrations of reactants and products
3 At equilibrium, the rate of the forward reaction is twice the rate of the backward reaction
4 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ for the reaction $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \text { is, } \frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]}$
Explanation:
(a) Equilibrium constant is temperature dependent having one unique value for a particular reaction represented by a balanced equation at a given temperature. (b) The value of equilibrium constant is independent of initial concentration of the reactants and products. (c) At equilibrium, the rate of forward reaction is equal to the rate of backward reaction. (d) For the equilibrium reaction- $\begin{array}{ll} & \mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \\ \therefore & \mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]^{4}} \end{array}$
TS-EAMCET-2016
Chemical Equilibrium
229169
Consider the following reaction $\mathrm{CaCO}_{3}(\mathrm{~s})$ $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ in closed container at equilibrium. What would be the effect of addition of $\mathrm{CaCO}_{3}$ on the equilibrium concentration of $\mathrm{CO}_{2}$ ?
229171
In a reaction, $A+B \rightleftharpoons C+D, 40 \%$ of $B$ has reacted at equilibrium, when 1 mole of $A$ was heated with 1 mole of $B$ in a $10 \mathrm{~L}$ closed vessel. The value of $K_{c}$ is
229180
The value of $\Delta H$ for the reaction $\mathbf{X}_{2}(\mathrm{~g})+\mathbf{4} \mathbf{Y}_{2}(\mathrm{~g}) \rightleftharpoons \mathbf{2} \mathbf{X Y}_{4}(\mathrm{~g})$ is less than zero formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at
1 high temperature and high pressure
2 low pressure and low temperature
3 high temperature and low pressure
4 high pressure and low temperature
Explanation:
The reaction is: $\begin{aligned} & \mathrm{X}_{2}(\mathrm{~g})+4 \mathrm{Y}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{XY}_{4}(\mathrm{~g}) \\ & \Delta \mathrm{n}_{\mathrm{g}}=-\mathrm{Ve} \end{aligned}$ And, $\quad \Delta \mathrm{H}=-\mathrm{Ve}$ So, formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at high pressure and low temperature.
229163
The chemical reaction of a gas phase is given below. $\mathbf{2 A}(\mathrm{g})+\mathbf{B}(\mathrm{g}) \rightleftharpoons \mathbf{C}(\mathrm{g})+\mathrm{D}(\mathrm{g})$ Which one of the following changes will affect the value of $K_{c}$ ?
1 Addition of inert gas
2 Increasing in temperature
3 Addition of reactants
4 Addition of catalyst
Explanation:
According to Vant Hoff equation- $\log \frac{\mathrm{K}_{2}}{\mathrm{~K}_{1}}=\frac{\Delta \mathrm{H}}{2.303 \mathrm{R}}\left(\frac{1}{\mathrm{~T}_{1}}-\frac{1}{\mathrm{~T}_{2}}\right)$ If, $\Delta \mathrm{H}$ is positive then the reaction is endothermic then temperature increase also the $\mathrm{K}$ is increases. $\Delta \mathrm{H}$ is negative then the reaction is exothermic then temperature increases also $\mathrm{K}$ is decreases. $\mathrm{K}_{\mathrm{c}}$ is a function of temperature only.
Manipal-2016
Chemical Equilibrium
229165
Which one of the following is correct?
1 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ is independent of temperature
2 The value of $K_{c}$ is independent of initial concentrations of reactants and products
3 At equilibrium, the rate of the forward reaction is twice the rate of the backward reaction
4 The equilibrium constant $\left(\mathrm{K}_{\mathrm{c}}\right)$ for the reaction $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \text { is, } \frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]}$
Explanation:
(a) Equilibrium constant is temperature dependent having one unique value for a particular reaction represented by a balanced equation at a given temperature. (b) The value of equilibrium constant is independent of initial concentration of the reactants and products. (c) At equilibrium, the rate of forward reaction is equal to the rate of backward reaction. (d) For the equilibrium reaction- $\begin{array}{ll} & \mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \\ \therefore & \mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]}{[\mathrm{CO}]^{4}} \end{array}$
TS-EAMCET-2016
Chemical Equilibrium
229169
Consider the following reaction $\mathrm{CaCO}_{3}(\mathrm{~s})$ $\mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ in closed container at equilibrium. What would be the effect of addition of $\mathrm{CaCO}_{3}$ on the equilibrium concentration of $\mathrm{CO}_{2}$ ?
229171
In a reaction, $A+B \rightleftharpoons C+D, 40 \%$ of $B$ has reacted at equilibrium, when 1 mole of $A$ was heated with 1 mole of $B$ in a $10 \mathrm{~L}$ closed vessel. The value of $K_{c}$ is
229180
The value of $\Delta H$ for the reaction $\mathbf{X}_{2}(\mathrm{~g})+\mathbf{4} \mathbf{Y}_{2}(\mathrm{~g}) \rightleftharpoons \mathbf{2} \mathbf{X Y}_{4}(\mathrm{~g})$ is less than zero formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at
1 high temperature and high pressure
2 low pressure and low temperature
3 high temperature and low pressure
4 high pressure and low temperature
Explanation:
The reaction is: $\begin{aligned} & \mathrm{X}_{2}(\mathrm{~g})+4 \mathrm{Y}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{XY}_{4}(\mathrm{~g}) \\ & \Delta \mathrm{n}_{\mathrm{g}}=-\mathrm{Ve} \end{aligned}$ And, $\quad \Delta \mathrm{H}=-\mathrm{Ve}$ So, formation of $\mathrm{XY}_{4}(\mathrm{~g})$ will favoured at high pressure and low temperature.
