33471
A reversible chemical reaction having two reactants in equilibrium. If the concentrations of the reactants are doubled, then the equilibrium constant will
1 Also be doubled
2 Be halved
3 Become one-fourth
4 Remain the same
Explanation:
(d)\({K_c}\) is a characteristic constant for the given reaction.
Chemical Equilibrium
33472
The equilibrium constant in a reversible reaction at a given temperature
1 Depends on the initial concentration of the reactants
2 Depends on the concentration of the products at equilibrium
3 Does not depend on the initial concentrations
4 It is not characteristic of the reaction
Explanation:
(c)Equilibrium constant is independent of original concentration of reactant.
Chemical Equilibrium
33473
Pure ammonia is placed in a vessel at temperature where its dissociation constant (\(\alpha \)) is appreciable. At equilibrium
1 \({K_p}\) does not change significantly with pressure
2 \(\alpha \) does not change with pressure
3 Concentration of \(N{H_3}\) does not change with pressure
4 Concentration of \({H_2}\) is less than that of \({N_2}\)
Explanation:
(a) \({K_p}\) is constant and does not change with pressure.
Chemical Equilibrium
33474
For the system \(A_{(g)} + 2B_{(g)}\) \(\rightleftharpoons\) \(C_{(g)}\), the equilibrium concentrations are \((A) 0.06\) mole/litre \((B) 0.12\) mole/litre \((C) 0.216\) mole/litre. The \({K_{eq}}\) for the reaction is
33471
A reversible chemical reaction having two reactants in equilibrium. If the concentrations of the reactants are doubled, then the equilibrium constant will
1 Also be doubled
2 Be halved
3 Become one-fourth
4 Remain the same
Explanation:
(d)\({K_c}\) is a characteristic constant for the given reaction.
Chemical Equilibrium
33472
The equilibrium constant in a reversible reaction at a given temperature
1 Depends on the initial concentration of the reactants
2 Depends on the concentration of the products at equilibrium
3 Does not depend on the initial concentrations
4 It is not characteristic of the reaction
Explanation:
(c)Equilibrium constant is independent of original concentration of reactant.
Chemical Equilibrium
33473
Pure ammonia is placed in a vessel at temperature where its dissociation constant (\(\alpha \)) is appreciable. At equilibrium
1 \({K_p}\) does not change significantly with pressure
2 \(\alpha \) does not change with pressure
3 Concentration of \(N{H_3}\) does not change with pressure
4 Concentration of \({H_2}\) is less than that of \({N_2}\)
Explanation:
(a) \({K_p}\) is constant and does not change with pressure.
Chemical Equilibrium
33474
For the system \(A_{(g)} + 2B_{(g)}\) \(\rightleftharpoons\) \(C_{(g)}\), the equilibrium concentrations are \((A) 0.06\) mole/litre \((B) 0.12\) mole/litre \((C) 0.216\) mole/litre. The \({K_{eq}}\) for the reaction is
33471
A reversible chemical reaction having two reactants in equilibrium. If the concentrations of the reactants are doubled, then the equilibrium constant will
1 Also be doubled
2 Be halved
3 Become one-fourth
4 Remain the same
Explanation:
(d)\({K_c}\) is a characteristic constant for the given reaction.
Chemical Equilibrium
33472
The equilibrium constant in a reversible reaction at a given temperature
1 Depends on the initial concentration of the reactants
2 Depends on the concentration of the products at equilibrium
3 Does not depend on the initial concentrations
4 It is not characteristic of the reaction
Explanation:
(c)Equilibrium constant is independent of original concentration of reactant.
Chemical Equilibrium
33473
Pure ammonia is placed in a vessel at temperature where its dissociation constant (\(\alpha \)) is appreciable. At equilibrium
1 \({K_p}\) does not change significantly with pressure
2 \(\alpha \) does not change with pressure
3 Concentration of \(N{H_3}\) does not change with pressure
4 Concentration of \({H_2}\) is less than that of \({N_2}\)
Explanation:
(a) \({K_p}\) is constant and does not change with pressure.
Chemical Equilibrium
33474
For the system \(A_{(g)} + 2B_{(g)}\) \(\rightleftharpoons\) \(C_{(g)}\), the equilibrium concentrations are \((A) 0.06\) mole/litre \((B) 0.12\) mole/litre \((C) 0.216\) mole/litre. The \({K_{eq}}\) for the reaction is
33471
A reversible chemical reaction having two reactants in equilibrium. If the concentrations of the reactants are doubled, then the equilibrium constant will
1 Also be doubled
2 Be halved
3 Become one-fourth
4 Remain the same
Explanation:
(d)\({K_c}\) is a characteristic constant for the given reaction.
Chemical Equilibrium
33472
The equilibrium constant in a reversible reaction at a given temperature
1 Depends on the initial concentration of the reactants
2 Depends on the concentration of the products at equilibrium
3 Does not depend on the initial concentrations
4 It is not characteristic of the reaction
Explanation:
(c)Equilibrium constant is independent of original concentration of reactant.
Chemical Equilibrium
33473
Pure ammonia is placed in a vessel at temperature where its dissociation constant (\(\alpha \)) is appreciable. At equilibrium
1 \({K_p}\) does not change significantly with pressure
2 \(\alpha \) does not change with pressure
3 Concentration of \(N{H_3}\) does not change with pressure
4 Concentration of \({H_2}\) is less than that of \({N_2}\)
Explanation:
(a) \({K_p}\) is constant and does not change with pressure.
Chemical Equilibrium
33474
For the system \(A_{(g)} + 2B_{(g)}\) \(\rightleftharpoons\) \(C_{(g)}\), the equilibrium concentrations are \((A) 0.06\) mole/litre \((B) 0.12\) mole/litre \((C) 0.216\) mole/litre. The \({K_{eq}}\) for the reaction is
