Question

Notify Me Bookmark

3.60 moles CO, 3.60 moles H2O, 1.00 moles CO2, and 1.00 moles H2 are put in a 2.00 L container at 600∘C. CO(g) + H2O(g) ⇄ CO2(g) + H2(g) Keq = 10.0 Calculate the equilibrium concentration of CO2. (4 marks)

3.60 moles CO, 3.60 moles H2O, 1.00 moles CO2, and 1.00 moles H2 are put in a 2.00 L container at 600∘C. CO(g) + H2O(g) ⇄ CO2(g) + H2(g) Keq = 10.0 Calculate the equilibrium concentration of CO2. (4 marks)

Image text
3.60 moles C O , 3.60 moles H 2 O , 1.00 moles C O 2 , and 1.00 moles H 2 are put in a 2.00 L container at 600 ∘ C .
C O ( g ) + H 2 O ( g ) ⇄ C O 2 ( g ) + H 2 ( g ) K e q = 10.0
Calculate the equilibrium concentration of C O 2 . (4 marks)

Detailed Answer

0 0

Please enter your email here. You will get email when this question is answered by our tutor.

Doubtrix Logo

Problem is not yet solved!

Click on Notify me to get email when question is answered.

Join Doubtrix with 7-days free trial

  • Icon Correct & Verified Answers
  • Icon No AI-Generated Answers
  • Icon Video Solution for Difficult Questions
  • Icon Work With Experts to Reach at Correct Answers
Notify me Login Sign Up

Similar/Related Questions

A mixture of 1.0 moles of H2 and 1.0 moles of I2 was placed in a 10.0 L flask at 700 K. The equilibrium constant for the reaction is 57.0. Calculate the concentration of HI at equilibrium. H2(g) + I2(g) "yields" 2HI(g) 0.079 M 0.021 M 1.0 M 0.16 M

Solution
0 0

1.6 mol of CH3OH (g) are injected into a 4.0 L container and the following equilibrium is established. 2H2 (g) + CO2 (g) ⇌ CH3OH (g) + 92 kJ a) At equilibrium, 0.80 mol of CH3OH is still in the container. Determine the equilibrium concentrations of all entities in mol/L. (4) b) Write the equilibrium law expression for this system. (1) c) Calculate the value of the equilibrium constant.
Solution
0 0

When 6.00 mol each of I2 (g), Br2 (g), and IBr (g) are placed in a 2.00 L vessel at constant temperature, they reach equilibrium according to the following equation: I2 (g) + Br2 (g) ⇌ 2 IBr (g) If Keq for this reaction is 0.683: a. Is this system at equilibrium? If not, which way will it shift to reach equilibrium? b. Determine the concentrations of all entities at equilibrium. Show all your steps.
Solution
0 0