Consider the following reaction where K 77.5 at 600 K. CO(g)+ Cl2g)COcl2(g) A re

Question

Consider the following reaction where K 77.5 at 600 K. CO(g)+ Cl2g)COcl2(g) A reaction mixture was found to contain 2.64x10% moles of CO(g), 4.08x10% moles of C12(g) and 0.107 moles of COC12(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe equals The reaction A. must run in the forward direction to reach equilibrium B. must run in the reverse direction to reach equilibrium. C. is at equilibrium

Explanation / Answer

since volume is 1 L, concentration will be same as number of moles

Qc = [COCl2] / [CO][Cl2]

= 0.107 / (2.64*10^-2 * 4.08*10^-2)

= 99.34

Since Qc is greater than Kc, the reaction will go in reverse direction

Answer:

Answer: Qc = 99.34

Answer: B

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

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