The following reaction is a reversible reaction. The value of Kc for this reaction is 31.4 at 588K.
CO(g) + H2O (g) 
CO2 (g) + H2 (g)
If a 10.00L vessel has 2.50 mol CO2 and H2O, and 5.00 mol CO2 and H2 gas at 588K, which way will the reaction proceed ?
Asked by Topperlearning User | 27th Apr, 2015, 04:15: PM
Expert Answer:
[CO] = .25 M
[H2O] = .25 M
[CO2] = .50 M
[H2] =.50 M
Hence, Qc = [CO2] [H2]/ [CO] [H2O] = 4
Since Qc < Kc, it will proceed in the forward direction.
Answered by | 27th Apr, 2015, 06:15: PM
Related Videos
- Define Le Chatelier's principle. How does it affect the equilibria.
- How does melting point decrease with increase in pressure for solid- liquid equillibrium . Pls explain using Le chattlier principle
- Im chemistry, what does it mean "the equilibrium state favours products or the reactants ? favored to what?
- What is Le Chatelier's principle?
- What are the factors which affect chemical equilibria?
- How Kc, KP, Qc and ΔGo are related?
- The following reaction is at equilibrium: 4NH3 (g) + 3O2 (g) 6H2O (g) + 2N2 (g) How will the equilibrium shift if: a) The volume is increased, b) Helium gas is added
- Define and explain the law of chemical equilibrium.
- Write equilibrium expressions for the following reversible reactions: 2 NO2 (g) N2O4 (g) N2 (g) + 3 H2 (g) 2 NH3 (g) 2 SO2 (g) + O2 (g) 2 SO3
Kindly Sign up for a personalised experience
- Ask Study Doubts
- Sample Papers
- Past Year Papers
- Textbook Solutions
Sign Up
Verify mobile number
Enter the OTP sent to your number
Change