The water gas shift reaction is an important industrial process for producing hy

Question

The water gas shift reaction is an important industrial process for producing hydrogen. Burning
coal provides both the cabon monoxide and the energy needed for this reaction.
CO(g) + H2O(g) ? CO2(g) + H2(g)
If 10.0 mol each of carbon monoxide and water were added to a 100.0 L flask at 500 K where the
equilibrium constant KC = 4.00, how much hydrogen would be produced? Note that you need not
use the quadratic formula to arrive at a solution if you are clever.
A) 6.7 mol
B) 7.6 mol
C) 2.0 mol
D) 20 mol
E) 6.3 mol

Explanation / Answer

CO(g) + H2O(g) --> CO2(g) + H2(g) ASSUME X MOLES OF CO REACTS WITH WATER [CO] = 10-X [H2O] = 10-X [CO2] = X [H2] = X SO, 4 = X^2/(10-X)^2 X = 20/3 MOLES SO, MOLES OF H2 PRODUCED WILL BE 20/3. ANSWER A) 6.7 mol IS CORRECT

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.