Question

The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g)...

The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction:
CO2(g) + H2(g) ⇌ CO(g) + H2O(g)
If 0.65 moles of CO2 and 0.65 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached?

The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction:
CO2(g) + H2(g) ⇌ CO(g) + H2O(g)
If 0.65 moles of CO2 and 0.65 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached?

0.30 M
0.38 M
0.42 M
0.35 M

Homework Answers

Answer #1

we know that

conc = moles / volume

given

volume = 1 L

so

conc = moles

so

initial conc of C02 = 0.65 M

initial conc of H2 = 0.65 M

the given reaction is

C02 + H2 ---> C0 + H20

the equilibrium constant is given by

Kc = [C0] [H20] / [C02] [H2]

now

consider the reaction

C02 + H2 ---> C0 + H20

using ICE table

initial conc of C02 , H2 , C0 , H20 are 0.65 ,0.65 , 0 , 0

change in conc of C02 , H2 , C0 , h20 are -x , -x ,+x , +x

equilibrium conc of C02 , H2 , CO , H20 are 0.65 -x , 0.65 - x , x ,x

now

Kc = [C0] [H20] / [C02] [H2]

1.4 = x2 / [0.65-x]^2

solving we get

x = 0.3523

now

[CO]eq = x

[C0]eq = 0.3523

so

the conc of CO at equilibrium is 0.35 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g)...
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached? The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of...
The Equilibrium constant Kc for the reaction H2(g) + CO2(g) -> H2O(g) + CO(g) is 4.2...
The Equilibrium constant Kc for the reaction H2(g) + CO2(g) -> H2O(g) + CO(g) is 4.2 at 1650 deg C. Initially .74 mol H2 and .74 mol CO2 are injected into a 4.6-L flask. Calculate the concentration of each species at equilibrium. H2= CO2 = H2O= CO=
The equilibrium constant Kc for the reaction H2(g) + CO2(g) = CO(g) + H20(g) is 5.1...
The equilibrium constant Kc for the reaction H2(g) + CO2(g) = CO(g) + H20(g) is 5.1 at 1700 C. Initially 0.65 mol of H2, 0.1 mol of CO and 0.65 mol of CO2 are injected into a 2.5-L flask. Calculate the concentraion of each species at equilibrium. Please show the steps so I can understand how to solve the problem. Thank you.
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730°...
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730° C. Starting with 4.20 moles of HBr in a 17.8−L reaction vessel, calculate the concentrations of H2,Br2, and HBr at equilibrium. 17. The equilibrium constant Kc for the reaction below is 0.00771 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0433 M and [Br] = 0.0462 M, calculate the concentrations of these species at equilibrium. For the reaction...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M COand 0.120 M H2O. A)What will be the equilibrium concentration of [CO]? B)What will be the equilibrium concentration of [H2O]? C)What will be the equilibrium concentration of [CO2]? D)What will be the equilibrium concentration of [H2]?
At a certain temperature, the equilibrium constant for the reaction CO2(g) + H2(g) <-> CO(g) +...
At a certain temperature, the equilibrium constant for the reaction CO2(g) + H2(g) <-> CO(g) + H2O(g) Is Kc = 5.45. If 4.00 mol of CO2 and 4.00 mol of H2 are placed in a 4.00 L vessel and equilibrium is established, what will be the concentration of water? a) 0.821 M b) 0.735 M c) 0.547 M d) 0.507 M e) 0.700 M I am very bad at math so please list all the steps so I can understand...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) +...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g) forward and reverse arrows 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.383 moles kf H2 and 0.383 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M [I2] = M [HI] = M
Consider the following reaction. CO (g) +H2O (g) = CO2 (g) + H2 (g) If the...
Consider the following reaction. CO (g) +H2O (g) = CO2 (g) + H2 (g) If the reaction begins in a 10.00 L vessel with 2.5 mol CO and 2.5 mol H2O gas at 588K (Kc= 31.4 at 588 K). Calculate the concentration of CO, H2O, CO2, and H2 at equilibrium.
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.306 moles of CO and 0.306 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is...
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is K = 49.0. A reaction mixture in a 10.00-L flask contains 0.25 moles each of hydrogen and fluorine gases plus 0.39 moles of HF. What will be the concentration of H2 when this mixture reaches equilibrium?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT