At 700 K, equilibrium constant for the reaction
`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?
Nitric oxide reacts with Br2 and gives nitrosyl bromide as per reaction given below:
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 equilibrium amount of NO and Br2 .
Write the expression for the equilibrium constant, Kc for following reactions:
Fe3+ (aq) + 3OH– (aq) ⇌ Fe(OH)3 (s)
A reaction between N2 and O2 takes place as follows:
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.
Predict which of the following reaction will have the appreciable concentration of reactants and products:
a) Cl2 (g) ⇌ 2Cl (g) Kc = 5 ×10–39
b) Cl2 (g) + 2NO (g) ⇌ 2NOCl (g) Kc = 3.7 × 108
c) Cl2 (g) + 2NO2 (g) ⇌ 2NO2Cl (g) Kc = 1.8
What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M?
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?
C2H6 (g) ⇌ C2H4 (g) + H2 (g)
The reaction, 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.