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प्रश्न
Write the expression for the equilibrium constant, Kc for each of the following reactions:
\[\ce{2NOCl (g) ⇌ 2NO (g) + Cl2 (g)}\]
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उत्तर
`"K"_"c" = (["NO"_(("g"))]^2["Cl"_(2("g"))])/["NOCl"_{("g")}]^2`
संबंधित प्रश्न
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 following reactions:
\[\ce{Fe^{3+}(aq) + 3OH^-(aq) ⇌ Fe(OH)3(s)}\]
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
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
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,
\[\ce{N2 + O2(g) ⇌ 2NO(g)}\]
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:
\[\ce{NO2(g) ⇌ 1/2 N2(g) + O2(g)}\]?
The stepwise formation of [Cu(NH3)4]2+ is given below:
\[\ce{Cu^{2+} + NH3 <=>[K1] [Cu(NH3)]^{2+}}\]
\[\ce{[Cu(NH3)]^{2+} + NH3 <=>[K2] [Cu(NH3)2]^{2+}}\]
\[\ce{[Cu(NH3)2]^{2+} + NH3 <=>[K3] [Cu(NH3)3]^{2+}}\]
\[\ce{[Cu(NH3)3]^{2+} + NH3 <=>[K4] [Cu(NH3)4]^{2+}}\]
The value of stability constants K1, K2, K3 and K4 are 104, 1.58 × 102, 5 × 103 and 102 respectively. The overall equilibrium constant for dissociation of [Cu(NH3)4]2+ is x × 10−12. The value of x is ______. (Rounded-off to the nearest integer)
For the reaction \[\ce{A(g) <=> B(g)}\] at 495 K, ΔG° = −9.478 kJ mol−1
If we start the reaction in a closed container at 495 K with 22 millimoles of A, the amount of B in the equilibrium mixture is ______ millimoles. (Round off to the Nearest Integer).
[R = 8.314 J mol−1 K−1; ln 10 = 2.303]
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 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 ______.
