At 100 degree C the equilibrium constant for the reaction below has the value of

Question

At 100 degree C the equilibrium constant for the reaction below has the value of K_eq = 2.19 times 10^-10. COCl_2(g) CO(g) Cl_2(g) Are the following mixtures of COCl_2, CO, and Cl_2 at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. (i) P_COCl_2 = 5.00 times 10^-2 atm: P_CO = 3.31 times 10^-6 atm: P_Cl_2 = 3.31 times 10^-6 atm (ii) P_COCl_2 = 3.50 times 10^-3 atm: P_CO = 1.11 times 10^-5 atm: P_Cl_2 = 3.25 times 10^-6 atm (i) equilibrium, (ii) not at equilibrium, right to left (ii) not at equilibrium, left to right, (ii) equilibrium (i) equilibrium, (ii) not at equilibrium, left to right (i) equilibrium, (ii) equilibrium (i)not at equilibrium, right to left, (ii) equilibrium

Explanation / Answer

Keq = 2.19*10^-10

i)

Qeq = p(CO)*p(Cl2)/p(COCl2)

= (3.31*10^-6)*(3.31*10^-6)/(5.00*10^-2)

= 2.19*10^-10

Since Qeq is equal to Keq, the system is already at equilibrium

ii)

Qeq = p(CO)*p(Cl2)/p(COCl2)

= (1.11*10^-5)*(3.25*10^-6)/(3.50*10^-3)

= 1.03*10^-8

Since Qeq is more than Keq, the system will move to left

Answer: i

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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