In the primary stage, a mixture of steam and methane at about 30 atm is heated over a nickel catalyst at 800°C to give hydrogen and carbon monoxide: CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g) ΔH°=260 kJ/mol The secondary stage is carried out at about 1000°C, in the presence of air, to convert the remaining methane to hydrogen: CH4 (g) + 1/2 O2 (g) ⇌ CO (g) + 2 H2 (g) ΔH°=35.7 kJ/mol (a) What conditions of temperature and pressure would favor the formation of products in both the primary and secondary stage? (b) The equilibrium constant Kc for the primary stage is 18 at 800°C. Calculate Kp for the reaction. (c) If the partial pressures of methane and steam were both 15 atm at the start, what are the pressures of all the gases at equilibrium?
In the primary stage, a mixture of steam and methane at about 30 atm is heated over a nickel catalyst at 800°C to give hydrogen and carbon monoxide:
CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g)
ΔH°=260 kJ/mol
The secondary stage is carried out at about 1000°C, in the presence of air, to convert the remaining methane to hydrogen:
CH4 (g) + 1/2 O2 (g) ⇌ CO (g) + 2 H2 (g)
ΔH°=35.7 kJ/mol
(a) What conditions of temperature and pressure would favor the formation of products in both the primary and secondary stage? (b) The equilibrium constant Kc for the primary stage is 18 at 800°C. Calculate Kp for the reaction. (c) If the partial pressures of methane and steam were both 15 atm at the start, what are the pressures of all the gases at equilibrium?
Thank you so much!
CH4 (g) + H2O (g) ⇌ CO (g) + 3H2 (g)
CH4 (g) + 1/2 O2 (g) ⇌ CO (g) + 2 H2 (g)
Kp = Kc (RT)Δn
where Kp = equilibrium constant when concentrations are measured in atmospheric pressure of gases
KC = quilibrium constant when concentrations are measured in molarity
Δn = change in the number of gaseous moles from reactant to product
R = gas constant
t= temperature
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
