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Question
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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Solution
`"K"_"c" = (["NO"_(("g"))]^2["Cl"_(2("g"))])/["NOCl"_{("g")}]^2`
RELATED QUESTIONS
Write the expression for the equilibrium constant, Kc for the following reactions:
\[\ce{2Cu(NO3)2 (s) ⇌ 2CuO (s) + 4NO2 (g) + O2 (g)}\]
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.
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,
\[\ce{H2O (g) + CO (g) ⇌ H2 (g) + CO2 (g)}\]
Calculate the equilibrium constant for the reaction.
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
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?
\[\ce{3Fe (s) + 4H2O (g) ⇌ Fe3O4 (s) + 4H2 (g)}\]
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?
At 500 K, equilibrium constant, \[\ce{K_c}\], for the following reaction is 5.
\[\ce{1/2 H2 (g) + 1/2 I2 (g) ⇌ HI (g)}\]
What would be the equilibrium constant \[\ce{K_c}\] for the reaction
\[\ce{2HI (g) ⇌ H2 (g) + I2 (g)}\]
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` |
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)
At 1990 K and 1 atm pressure, there are equal numbers of Cl2 molecules and Cl atoms in the reaction mixture. The value of Kp for the reaction Cl2(g) ⇌ 2Cl(g) under the above conditions is x × 10−1. 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:
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
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 ______.
In which of the following equilibria, Kp and Kc are not equal?
