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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

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प्रश्न

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
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उत्तर

Column I Column II
(i) ∆GΘ > 0 (d) K < 1
(ii) ∆GΘ > 0  (a) K > 1
(iii) ∆GΘ = 0 (b) K = 1
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Law of Chemical Equilibrium and Equilibrium Constant
  या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?
पाठ 7: Equilibrium - Multiple Choice Questions (Type - I) [पृष्ठ ९३]

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एनसीईआरटी एक्झांप्लर Chemistry [English] Class 11
पाठ 7 Equilibrium
Multiple Choice Questions (Type - I) | Q 40 | पृष्ठ ९३

संबंधित प्रश्‍न

What is Kc for the following equilibrium when the equilibrium concentration of each substance is: [SO2] = 0.60 M, [O2] = 0.82 M and [SO3] = 1.90 M?

\[\ce{2SO2(g) + O2(g) ⇌ 2SO3(g)}\]


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 following reactions:

\[\ce{Fe^{3+}(aq) + 3OH^-(aq) ⇌ Fe(OH)3(s)}\]


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

\[\ce{I2 (s) + 5F2 ⇌ 2IF5}\]


A reaction between N2 and O2 takes place as follows:

\[\ce{2N2 (g) + O2 (g) ⇌ 2N2O (g)}\]

If a mixture of 0.482 mol of N2 and 0.933 mol of O2 is placed in a 10 L reaction vessel and allowed to form N2O at a temperature for which Kc = 2.0 × 10-37, determine the composition of equilibrium mixture.


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?


What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M?

\[\ce{2 ICl(g) ⇌  I2(g) + Cl2(g)}\]; KC = 0.14


Kp = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C2H6 when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

\[\ce{C2H6 (g) ⇌ C2H4 (g) + H2 (g)}\]


Calculate a) ΔG°and b) the equilibrium constant for the formation of NO2 from NO and O2 at 298 K

\[\ce{NO(g) + 1/2 O_2 (g) <=> NO_2(g)}\]

where ΔfG (NO2) = 52.0 kJ/mol

ΔfG (NO) = 87.0 kJ/mol

ΔfG (O2) = 0 kJ/mol


Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?

\[\ce{3Fe (s) + 4H2O (g) ⇌ Fe3O4 (s) + 4H2 (g)}\]


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`

An equilibrium system for the reaction between hydrogen and iodine to give hydrogen iodide at 765 K in a 5 litre volume contains 0.4 mole of hydrogen, 0.4 mole of iodine and 2.4 moles of hydrogen iodide.

\[\ce{H2 + I2 <=> 2HI}\]

The equilibrium constant for the reaction is:


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 equilibrium constant for the reaction is ______ × 1026.

\[\ce{Fe + CuSO4 <=> FeSO4 + Cu}\] at 25°C.

Given `"E"_("Fe"//"Fe"^(2+))^0` = 0.44 V

`"E"_("Cu"//"Cu"^(2+))^0` = - 0.337 V


The value of Kc is 64 at 800 K for the reaction \[\ce{N2(g) + 3H2(g) <=> 2NH3(g)}\].

The value of Kc for the following reaction is:

\[\ce{NH3(g) <=> 1/2N2(g) + 3/2H2(g)}\]


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 ______.


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