In the manufacture of ammonia, the chief source of hydrogen gas is the reaction for the reforming of methane at high temperatures.
CH4(g)+2H2O (arrows) CO2(g)+H2(g) (overall reaction)
The following data is also given.
1) CO(g)+H2O(g) (arrows) CO2(g)+H2(g)
H= -40kJ Keq=1.4
2) CO(g)+3H2(g) (arrows)H2O(g)+CH4(g)
H= -230kJ Keq= 190
A mixture containing 1.00mol of each of CH4(g) and H2O(g) is brought to equilibrium in the overall reaction in a 10.0L flask. The equilibrium mixture is found to contain 12.4g of unreacted CH4(g).
a) Calculate the mass of H2(g) also present at equilibrium.
b) Describe the effect on the equilibrium amount of H2 produced by each of these actions:
1) Add CH4 (increase)
2) Add CO2 (decrease)
3) Add He(g) at constant volume (increase)
4) Remove H2O (decrease)
5) Raise the temperature (increase)
6) Transfer the mixture to a 15.0L flask (increase)
I didn't get part a and part b I'm not sure about my answers but can someone check them to see if their right?
CH4(g)+2H2O (arrows) CO2(g)+H2(g) (overall reaction)
The following data is also given.
1) CO(g)+H2O(g) (arrows) CO2(g)+H2(g)
H= -40kJ Keq=1.4
2) CO(g)+3H2(g) (arrows)H2O(g)+CH4(g)
H= -230kJ Keq= 190
A mixture containing 1.00mol of each of CH4(g) and H2O(g) is brought to equilibrium in the overall reaction in a 10.0L flask. The equilibrium mixture is found to contain 12.4g of unreacted CH4(g).
a) Calculate the mass of H2(g) also present at equilibrium.
b) Describe the effect on the equilibrium amount of H2 produced by each of these actions:
1) Add CH4 (increase)
2) Add CO2 (decrease)
3) Add He(g) at constant volume (increase)
4) Remove H2O (decrease)
5) Raise the temperature (increase)
6) Transfer the mixture to a 15.0L flask (increase)
I didn't get part a and part b I'm not sure about my answers but can someone check them to see if their right?