Hydrogen and carbon dioxide gases are mixed at 800K. A reversible reaction takes place.
H2(g) + CO2(g)==> H2O(g) + CO(g)
At equilibrium, the partial pressures of H2 and CO2 are both 10.0 kPa. Kp is 0.288 at 800K.
What is the partial pressure of CO in the equilibrium mixture?
A 5.37 kPa B 18.6 kPa C 28.8 kPa D 347 kPa
Answer scheme says it's A. Can someone please show me the working?
Turn on thread page Beta
CIE A-levels Chemistry watch
- Thread Starter
- 07-11-2017 10:36
- Official Rep
- 09-11-2017 14:16
Sorry you've not had any responses about this. Are you sure you've posted in the right place? Here's a link to our subject forum which should help get you more responses if you post there.
- 14-11-2017 11:47
Kp= (partial pressure of CO x parital pressure of H20) / (partial pressure of CO2 x partial pressure of H2
• Since the moles of CO2 and H2 are same, and they have equal partial pressures, we assume that the partial pressures of the two products will also be same since they too have the same number of moles
Kp = p(CO) x p(H2O) / p(CO2) x p(H2)
0.288= (p x p) / 10 x 10
0.288= p^2 / 100
0.288 x 100= p^2
28.8 = p^2
_/28.8 = _/p^2
5.366 = p
p ~ 5.37kPa
So answer is ALast edited by Big dreams; 14-11-2017 at 11:52.