Question 12
0.2 / 0.2 pts
At temperatures near 800 °C, steam passed over hot coke (a form of carbon obtained from coal) reacts to form
CO and H$_2$:
C(s) + H$_2$O(g) <--> CO(g) + H$_2$(g)
The mixture of gases that results is an important industrial fuel called water gas. At 800 °C the equilibrium
constant for this reaction is Kp = 14.1. What are the equilibrium partial pressures in atm of H$_2$O, CO, and H$_2$ in the
equilibrium mixture at this temperature if we start with excess solid carbon and 0.200 mol of H$_2$O in a 1.00-L
vessel?
P$_{CO}$ = 6.14, P$_{H_2}$ = 10.2, P$_{H_2O}$ = 6.14
P$_{CO}$ = 10.2, P$_{H_2}$ = 10.2, P$_{H_2O}$ = 10.2
P$_{CO}$ = 10.2, P$_{H_2}$ = 10.2, P$_{H_2O}$ = 7.40
P$_{CO}$ = 7.4, P$_{H_2}$ = 10.2, P$_{H_2O}$ = 7.40
P$_{CO}$ = 10.2, P$_{H_2}$ = 7.4, P$_{H_2O}$ = 7.40
