47. At high temperatures carbon dioxide reacts with hydrogen CO2(g) + H2(g)CO(g)

Question

47. At high temperatures carbon dioxide reacts with hydrogen CO2(g) + H2(g)CO(g) + H2O(g) Kp = 1.4 at 1 100 K At 1100 K. the initial pressures of carbon dioxide and hydrogen are both 5.0 atm and the initial pressures of carbon monoxide and water vapor are both 4.0 atm. a. In which direction must the reaction proceed in order to reach equilibrium? b. What are the equilibrium partial pressures of each gas? c. What is the total pressure after equilibrium is reached? What is the mole fraction of carbon monoxide after equilibrium is reached?

Explanation / Answer

a. Since Kp = 1.4, i.e. >1, the reaction slightly shifts to right side. Hence, the reaction must proceed towards the left side to reach the equilibrium.

b. Cp = (PCO * PH2O)/(PCO2 * PH2O)

i.e. 1.4 = (5-x)*(5-x)/(4+x)*(4+x)

i.e. x2 - 2x + 25 = 1.4* (x2 + 2x + 16)

i.e. 0.4 x2 + 4.8x - 2.6 = 0

i.e. 0.2 x2 + 2.4 x - 1.3 = 0

i.e. x = 0.52

Therefore, the equilirbrium partical pressure of CO2 and H2 = 5-0.519 = 4.48

And the equilirbrium partical pressure of CO and H2O = 4+0.52 = 4.52

c. The total pressure after equilibrium is reached = 2*4.48 + 2*4.52 = 18 atm

The mole fraction of CO2 = PCO2/P = 4.48/18 = 0.249 ~ 0.25

Related Questions

Navigate

• Browse (All)
• Browse 4
• Subjects

---

---

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