Chemical Equilibrium

Given below are certain reactions. Identify the reaction for which $K_P \neq K_C$.

Higher yield of NO in $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})$ can be obtained at $\left[\Delta \mathrm{H}\right.$ of the reaction $\left.=+180.7 \mathrm{~kJ} \mathrm{~mol}^{-1}\righ...

For the reaction $\mathrm{A}(\mathrm{g}) \rightleftharpoons 2 \mathrm{~B}(\mathrm{~g})$, the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500 , at 1000 K.
[Given : $\mathrm{R}=0.0831 \mat...

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:

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 \math...

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 \math...

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, whi...

In which of the following equilibria, \(\mathrm{K}_p\) and \(\mathrm{K}_{\mathrm{c}}\) are NOT equal?

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

Which one of the following conditions will
favour maximum formation of the product in
the reaction
A2(g)
+ B2(g) ⇌ X2(g)
, \(\Delta\)rH = –X kJ ?

The equilibrium constants of the following are
N2 + 3H2 \(\rightleftharpoons\) 2NH3;     K1
N2 + O2 \(\rightleftharpoons\) 2NO;     K2
H2 + \({1 \over 2}\)O2 \(\rightleftharpoons\)
H2O;     K3
The equilibrium constant (K) of the rea...

A 20 litre container at 400 K contains CO2(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume...

Consider the following liquid-vapour equilibrium.
Liquid \(\rightleftharpoons\) Vapour
Which of the following relations is correct ?

If the value of equilibrium constant for a particular reaction is 1.6 \(\times\) 1012, then at equilibrium the system will contain

Which of the following statements is correct for a reversible process in a state of equilibrium?

If the equilibrium constant for
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

For the reversible reaction,
N2(g) + 3H2(g) \(\rightleftharpoons\) 2NH3(g) + heat
The equilibrium shifts in forward direction

For a given exothermic reaction, Kp and K'p are the equilibrium constants at temperatures T1 and T2, respectively. Assuming that heat of reaction is constant in temperature range between T1 and T2, it is readily observed that

Using the Gibb's energy change, \(\Delta\)Go = +63.3 kJ, for the following reaction,
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)

Given that the equilibrium constant for the reaction,
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 temp...

Given the reaction between 2 gases represented by A2 and B2 to give the compound AB(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\(-\)...

For the reaction, N2(g) + O2(g) \(\rightleftharpoons\) 2NO(g), the equilibrium constant is K1. The equilibrium constant is K2 for the reaction,
2NO(g) + O2(g) \(\rightleftharpoons\) 2NO2(g)
What is K for the reaction,
NO2(g) $$\rightleft...

The value of \(\Delta\)H for the reaction
X2(g) + 4Y2(g) \(\rightleftharpoons\) 2XY4(g)
is less than zero. Formation of XY4(g) will be favoured at

In which of the following equilibrium Kc and Kp are not equal?

The reaction,
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 v...

The dissociation constants for acetic acid and HCN at 25oC are 1.5 \(\times\) 10\(-\)5 and 4.5 \(\times\) 10\(-\)10 respectively. The equilibrium constant for the equilibrium
CN\(-\) + CH3COOH \(\rightleftharpoons\) HCN + CH3COO$$-$...

The values of for the reactions,
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)...

The dissociation equilibrium of a gass AB2 can be represented as :
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 equil...

If the concentration of OH\(-\) ions in the reaction
Fe(OH)3(s) \(\rightleftharpoons\) Fe3+(aq) + 3OH\(-\)(aq)
is decreased by 1/4 times, then equilibrium concentration of Fe3+ will increase by

The value of equilibrium constant of the reaction
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

The equilibrium constants of the following are
N2 + 3H2 \(\rightleftharpoons\) 2NH3;     K1
N2 + O2 \(\rightleftharpoons\) 2NO;     K2
H2 + \({1 \over 2}\)O2 \(\rightleftharpoons\)
H2O;     K3
The equilibrium constant (K) of the rea...

For the reaction :
CH4(g) + 2O2(g) \(\rightleftharpoons\) CO2(g) + 2H2O(l),
\(\Delta\)Hr = \(-\) 170.8 kJ mol\(-\)1.
Which of the following statements is not true?

Equilibrium constants K1 and K2 for the following equilibriam:

are related as

The equilibrium constants of the following are
N2 + 3H2 \(\rightleftharpoons\) 2NH3;     K1
N2 + O2 \(\rightleftharpoons\) 2NO;     K2
H2 + \({1 \over 2}\)O2 \(\rightleftharpoons\)
H2O;     K3
The equilibrium constant (K) of the rea...

The reaction quotient (Q) for the reaction 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 rig...

Reaction BaO2(g) \(\rightleftharpoons\) BaO(s) + O2(g); \(\Delta\)H = +ve. In equilibrium condition, pressure of O2 depends on

Equilibrium constant Kp for following reaction
MgCO3(s) \(\rightleftharpoons\) MgO(s) + CO2(g)

For any reversible reaction, if we increase concentration of the reactants, then effect on equilibrium constant