3 (i) In the Haber process for the production of ammonia, the following reaction occurs: N2 (g) + 3H2 (g) 2NH3 (g) DH is negative If the equilibrium concentrations for all the reactants and products at 6000C are: [N2] = 0.40 mol/dm3, [H2] = 1.20 mol/dm3 and [NH3] = 0.20 mol/ dm3 Construct an expression for Kc and calculate the numerical value of the equilibrium constant, Kc (ii) At 5000C Kc = 0.062 mol-2dm6. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 5000C or 6000C and briefly explain your choice.
3 (i) In the Haber process for the production of ammonia, the following reaction occurs:
N2 (g) + 3H2 (g) 2NH3 (g) DH is negative
If the equilibrium concentrations for all the reactants and products at 6000C are:
[N2] = 0.40 mol/dm3, [H2] = 1.20 mol/dm3 and [NH3] = 0.20 mol/ dm3
Construct an expression for Kc and calculate the numerical value of the equilibrium constant, Kc
(ii) At 5000C Kc = 0.062 mol-2dm6. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 5000C or 6000C and briefly explain your choice.
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