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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 - Chemistry

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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

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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 the following reactions:

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


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


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

\[\ce{I2 (s) + 5F2 ⇌ 2IF5}\]


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\[\ce{2N2 (g) + O2 (g) ⇌ 2N2O (g)}\]

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.


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\[\ce{2NO(g) + Br2 (g) ⇌ 2NOBr (g)}\]

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One mole of H2O and one mole of CO are taken in 10 L vessel and heated to 725 K. At equilibrium, 40% of water (by mass) reacts with CO according to the equation, 

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

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?

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Predict which of the following reaction will have the appreciable concentration of reactants and products:

  1. \[\ce{Cl2 (g) ⇌ 2Cl (g)}\] Kc = 5 ×10–39
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\[\ce{N2 + O2(g) ⇌ 2NO(g)}\]

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:

\[\ce{NO2(g) ⇌ 1/2 N2(g) + O2(g)}\]?


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

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


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