English
Karnataka Board PUCPUC Science Class 11

Match standard free energy of the reaction with the corresponding equilibrium constant. Column I Column II (i) ∆GΘ > 0 (a) K > 1 (ii) ∆GΘ > 0 (b) K = 1 (iii) ∆GΘ = 0 (c) K = 0 (d) K < 1

Advertisements
Advertisements

Question

Match standard free energy of the reaction with the corresponding equilibrium constant.

Column I Column II
(i) ∆GΘ > 0 (a) K > 1
(ii) ∆GΘ > 0  (b) K = 1
(iii) ∆GΘ = 0 (c) K = 0
  (d) K < 1
Match the Columns
Advertisements

Solution

Column I Column II
(i) ∆GΘ > 0 (d) K < 1
(ii) ∆GΘ > 0  (a) K > 1
(iii) ∆GΘ = 0 (b) K = 1
shaalaa.com
Law of Chemical Equilibrium and Equilibrium Constant
  Is there an error in this question or solution?
Chapter 7: Equilibrium - Multiple Choice Questions (Type - I) [Page 93]

APPEARS IN

NCERT Exemplar Chemistry Exemplar [English] Class 11
Chapter 7 Equilibrium
Multiple Choice Questions (Type - I) | Q 40 | Page 93

RELATED QUESTIONS

Write the expression for the equilibrium constant, Kc for each of the following reactions:

\[\ce{2NOCl (g) ⇌ 2NO (g) + Cl2 (g)}\]


Write the expression for the equilibrium constant, Kc for the following reactions:

\[\ce{2Cu(NO3)2 (s) ⇌ 2CuO (s) + 4NO2 (g) + O2 (g)}\]


Write the expression for the equilibrium constant, Kc for the following reactions:

\[\ce{CH3COOC2H5(aq) + H2O(l) ⇌CH3COOH (aq) + C2H5OH (aq)}\]


Write the expression for the equilibrium constant, Kc for the following reactions

\[\ce{I2 (s) + 5F2 ⇌ 2IF5}\]


Nitric oxide reacts with Br2 and gives nitrosyl bromide as per reaction given below:

\[\ce{2NO(g) + Br2 (g) ⇌ 2NOBr (g)}\]

When 0.087 mol of NO and 0.0437 mol of Br2 are mixed in a closed container at the constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate the equilibrium amount of NO and Br2.


At 700 K, the equilibrium constant for the reaction

\[\ce{H_{2(g)} + I_{2(g)} ↔ 2HI_{(g)}}\] 

is 54.8. If 0.5 molL–1 of HI(g) is present at equilibrium at 700 K, what are the concentration of H2(g) and I2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K?


The reaction, \[\ce{CO(g) + 3H2(g) ↔ CH4(g) + H2O(g)}\] is at equilibrium at 1300 K in a 1L flask. It also contains 0.30 mol of CO, 0.10 mol of H2 and 0.02 mol of H2O and an unknown amount of CH4 in the flask. Determine the concentration of CH4 in the mixture. The equilibrium constant, Kc for the reaction at the given temperature is 3.90.


For the reaction \[\ce{H2 (g) + I2 (g) ⇌ 2HI (g)}\], the standard free energy is  ∆GΘ > 0. The equilibrium constant (K ) would be ______.


On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.

\[\ce{N2 (g) + 3H2 (g) ⇌ 2NH3 (g)}\]

Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?


For the reaction : \[\ce{N2 (g) + 3H2 (g) ⇌ 2NH3 (g)}\]

Equilibrium constant `K_C = ([NH3]^2)/([N_2][H_2]^3)`

Some reactions are written below in Column I and their equilibrium constants in terms of Kc are written in Column II. Match the following reactions with the corresponding equilibrium constant

Column I (Reaction) Column II (Equilibrium constant)
(i) \[\ce{2N2 (g) + 6H2 (g) ⇌ 4NH3 (g)}\] (a) `2K_c`
(ii) \[\ce{2NH3 (g) ⇌ N2 (g) + 3H2 (g)}\] (b) `K_c^(1/2)`
(iii) \[\ce{1/2 N2 (g) + 3/2 H2 (g) ⇌ NH3 (g)}\] (c) `1/K_c`
  (d) `K_c^2`

For the reaction,

\[\ce{N2 + O2(g) ⇌ 2NO(g)}\]

the equilibrium constant is K1. The equilibrium constant is K2 for the reaction

\[\ce{2NO(g) + O2(g) ⇌ 2NO2(g)}\]

What is "K" for the reaction:

\[\ce{NO2(g) ⇌ 1/2 N2(g) + O2(g)}\]?


Sulphide ion in alkaline solution reacts with solid sulphur to form polysulphide ions having formula, \[\ce{S^{2-}2}\], \[\ce{S^{2-}3}\], \[\ce{S^{2-}4}\], etc. if K1 = 12 for \[\ce{S + S^{2-} <=> S^{2-}2}\] and K2 = 132 for \[\ce{2S + S^{2-} <=> S^{2-}3}\], K3 = ______ for \[\ce{S + S^{2-}2 <=> S^{2-}3}\].


The decomposition of N2O4 to NO2 was carried out in chloroform at 280°C. At equilibrium, 0.2 mol of N2O4 and 2 × 10−3 mol of NO2 were present in 2 ℓ of the solution. The equilibrium constant for the reaction \[\ce{N2O4 <=> 2NO2}\] is ______.


In which one of the following equilibria, KP ≠ Kc?


A solid XY kept in an evacuated sealed container undergoes decomposition to form a mixture of gases X and Y at temperature T. The equilibrium pressure is 10 bar in the vessel. Kp for this reaction is ______.


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×