Chemical Equilibrium · Chemistry · NEET
MCQ (Single Correct Answer)
At a given temperature and pressure, the equilibrium constant values for the equilibria are given below:
$$\begin{aligned} & 3 \mathrm{~A}_2+\mathrm{B}_2 \rightleftharpoons 2 \mathrm{~A}_3 \mathrm{~B}, \mathrm{~K}_1 \\ & \mathrm{~A}_3 \mathrm{~B} \rightleftharpoons \frac{3}{2} \mathrm{~A}_2+\frac{1}{2} \mathrm{~B}_2, \mathrm{~K}_2 \end{aligned}$$
The relation between $$\mathrm{K}_1$$ and $$\mathrm{K}_2$$ is :
For the reaction in equilibrium
$$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}), \Delta \mathrm{H}=-\mathrm{Q}$$
Reaction is favoured in forward direction by:
In which of the following equilibria, $$\mathrm{K}_p$$ and $$\mathrm{K}_{\mathrm{c}}$$ are NOT equal?
For the reaction $$2 \mathrm{~A} \rightleftharpoons \mathrm{B}+\mathrm{C}, \mathrm{K}_{\mathrm{c}}=4 \times 10^{-3}$$. At a given time, the composition of reaction mixture is: $$[A]=[B]=[C]=2 \times 10^{-3} \mathrm{M} \text {. }$$ Then, which of the following is correct?
Consider the following reaction in a sealed vessel at equilibrium with concentrations of $$\mathrm{N}_2=3.0 \times 10^{-3} \mathrm{M}, \mathrm{O}_2=4.2 \times 10^{-3} \mathrm{M}$$ and $$\mathrm{NO}=2.8 \times 10^{-3} \mathrm{M}$$.
$$2 \mathrm{NO}_{(\mathrm{g})} \rightleftharpoons \mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$$
If $$0.1 \mathrm{~mol} \mathrm{~L} \mathrm{~L}^{-1}$$ of $$\mathrm{NO}_{(\mathrm{g})}$$ is taken in a closed vessel, what will be degree of dissociation ($$\alpha$$) of $$\mathrm{NO}_{(\mathrm{g})}$$ at equilibrium?
For a weak acid HA, the percentage of dissociation is nearly 1% at equilibrium. If the concentration of acid is 0.1 mol L$$^{-1}$$, then the correct option for its K$$_a$$ at the same temperature is :
Kp for the following reaction is 3.0 at 1000 K.
CO2(g) + C(s) $$\rightleftharpoons$$ 2CO(g)
What will be the value of Kc for the reaction at the same temperature?
(Given : R = 0.083 L bar K$$-$$1 mol$$-$$1)
3O2(g) $$\rightleftharpoons$$ 2O3(g)
for the above reaction at 298 K, Kc is found to be 3.0 $$\times$$ 10$$-$$59. If the concentration of O2 at equilibrium is 0.040 M then concentration of O3 in M is
A2(g) + B2(g) ⇌ X2(g) , $$\Delta $$rH = –X kJ ?
N2 + 3H2 $$\rightleftharpoons$$ 2NH3; K1
N2 + O2 $$\rightleftharpoons$$ 2NO; K2
H2 + $${1 \over 2}$$O2 $$\rightleftharpoons$$ H2O; K3
The equilibrium constant (K) of the reaction :
2NH3 + $${5 \over 2}$$ O2 $$\rightleftharpoons$$ 2NO + 3H2O will be
(Given that : SrCO3(s) $$\rightleftharpoons$$ SrO(s) + CO2(g), Kp = 1.6 atm)
Liquid $$\rightleftharpoons$$ Vapour
Which of the following relations is correct ?
N2(g) + O2(g) $$\rightleftharpoons$$ 2NO(g) is K, the equilibrium
constant for
$${1 \over 2}$$ N2(g) + $${1 \over 2}$$O2(g) $$\rightleftharpoons$$ NO(g) will be
N2(g) + 3H2(g) $$\rightleftharpoons$$ 2NH3(g) + heat
The equilibrium shifts in forward direction
Ag2CO3(s) $$\rightleftharpoons$$ 2 Ag+(aq) + CO32$$-$$ (aq)
the Ksp of Ag2CO3(s) in water at 25oC is
(R = 8.314 J K$$-$$1 mol$$-$$1)
2SO2(g) + O2(g) $$\rightleftharpoons$$ 2SO3(g)
has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature ?
SO3(g) $$\rightleftharpoons$$ SO2(g) + $${1 \over 2}$$ O2(g)
A2(g) + B2(g) $$\rightleftharpoons$$ 2AB(g)
At equilibrium, the concentration of
A2 = 3.0 $$ \times $$ 10$$-$$3 M, of B2 = 4.2 $$ \times $$ 10$$-$$3 M, of AB = 2.8 $$ \times $$ 10$$-$$3 M
If the reaction takes place in a sealed vessel at 527oC, then the value of Kc will be
X2(g) + 4Y2(g) $$\rightleftharpoons$$ 2XY4(g)
is less than zero. Formation of XY4(g) will be favoured at
2NO(g) + O2(g) $$\rightleftharpoons$$ 2NO2(g)
What is K for the reaction,
NO2(g) $$\rightleftharpoons$$ $${1 \over 2}$$N2(g) + O2(g)
2A(g) + B(g) $$\rightleftharpoons$$ 3C(g) + D(g)
is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measuread and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression
CN$$-$$ + CH3COOH $$\rightleftharpoons$$ HCN + CH3COO$$-$$ would be
HI(g) $$\rightleftharpoons$$ $${1 \over 2}$$H2(g) + $${1 \over 2}$$I2(g)
is 8.0. The The equilibrium constant of the reaction
H2(g) + I2(g) $$\rightleftharpoons$$ 2HI(g) will be
X $$\rightleftharpoons$$ Y + Z . . . .(i)
A $$\rightleftharpoons$$ 2B . . . .(ii)
are in the ratio 9 : 1. If degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and (ii) are in the ratio
Fe(OH)3(s) $$\rightleftharpoons$$ Fe3+(aq) + 3OH$$-$$(aq)
is decreased by 1/4 times, then equilibrium concentration of Fe3+ will increase by
2AB2(g) $$\rightleftharpoons$$ 2AB(g) + B2(g)
The degree of dissociation is x and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant Kp and total pressure P is
N2 + 3H2 $$\rightleftharpoons$$ 2NH3; K1
N2 + O2 $$\rightleftharpoons$$ 2NO; K2
H2 + $${1 \over 2}$$O2 $$\rightleftharpoons$$ H2O; K3
The equilibrium constant (K) of the reaction :
2NH3 + $${5 \over 2}$$ O2 $$\rightleftharpoons$$ 2NO + 3H2O will be
CH4(g) + 2O2(g) $$\rightleftharpoons$$ CO2(g) + 2H2O(l),
$$\Delta $$Hr = $$-$$ 170.8 kJ mol$$-$$1.
Which of the following statements is not true?
are related as
N2 + 3H2 $$\rightleftharpoons$$ 2NH3; K1
N2 + O2 $$\rightleftharpoons$$ 2NO; K2
H2 + $${1 \over 2}$$O2 $$\rightleftharpoons$$ H2O; K3
The equilibrium constant (K) of the reaction :
2NH3 + $${5 \over 2}$$ O2 $$\rightleftharpoons$$ 2NO + 3H2O will be
N2(g) + 3H2(g) $$\rightleftharpoons$$ 2NH3(g) is given by
$$Q = {{{{\left[ {N{H_3}} \right]}^2}} \over {\left[ {{N_2}} \right]{{\left[ {{H_2}} \right]}^3}}}$$.
The reaction will proceed from right to left if
MgCO3(s) $$\rightleftharpoons$$ MgO(s) + CO2(g)