Advertisements
Advertisements
Question
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?
\[\ce{2SO2(g) + O2(g) ⇌ 2SO3(g)}\]
Advertisements
Solution
The equilibrium constant (Kc) for the give reaction is:
`"K"_"c" = ["SO"_3]^2/(["SO"_2]^2["O"_2])`
`= ((1.90)^2 "M"^2)/((0.60)^2 (0.821)"M"^3)`
`= 12.239 " M"^(-1) ("approximately")`
Hence, Kc for the equilibrium is `12.239 " M"^(-1)`
APPEARS IN
RELATED QUESTIONS
Write the expression for the equilibrium constant, Kc for each of the following reactions:
\[\ce{2NOCl (g) ⇌ 2NO (g) + Cl2 (g)}\]
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?
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
Predict which of the following reaction will have the appreciable concentration of reactants and products:
- \[\ce{Cl2 (g) ⇌ 2Cl (g)}\] Kc = 5 ×10–39
- \[\ce{Cl2 (g) + 2NO (g) ⇌ 2NOCl (g)}\] Kc = 3.7 × 108
- \[\ce{Cl2 (g) + 2NO2 (g) ⇌ 2NO2Cl (g)}\] Kc = 1.8
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?
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 |
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]
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 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 ______.
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?
