Question

The equilibrium constant for 2 CO2 (g) ⇌ 2 CO (g) + O2 (g) is 1.12x10-45...

The equilibrium constant for 2 CO2 (g) ⇌ 2 CO (g) + O2 (g) is 1.12x10-45 at room temperature. If the initial concentration of CO2 is 10 mM, what are the equilibrium concentrations of all three chemicals? The equilibrium constant is small, so you can assume x will be small.

Homework Answers

Answer #1

            2 CO2 (g) ⇌ 2 CO (g) + O2 (g)

Initial   10mM            0              0

Final   (10mM-2x)    2x              x

Keq = 1.12 * 10^(-45) = [CO]^2[O2]/[CO2]^2

1.12 * 10^(-45) = 4x^3/10mM (assuming 2x is very small as compared to x)

11.2 * 10^(-48) = 4x^3

x^3 = 2.8 * 10^(-48)

x = 1.4094 * 10^(-16) 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
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 for the following reaction in groundwater is about 1.5x10-56. If the initial...
. The equilibrium constant for the following reaction in groundwater is about 1.5x10-56. If the initial concentration of K+ was 12 mM and of H2 (aq) was 0.10 mM, what are the equilibrium concentrations expected? The equilibrium constant is very small, so you can assume x is small. 2 K+ (aq) + H2 (aq) ⇌ 2 K (aq) + 2 H+ (aq)
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI...
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI (b)2 NO(g) + O2(g)           2 NO2(g) (c)N2(g) + 3 H2(g)           2 NH3(g) (d) CO(g) + NO2(g)           CO2(g) + NO(g) (e) 2 CO(g) + O2(g)             2 CO2(g) 2.    Write equilibrium expressions for each of the following equilibria: (a) 2 C(s) + O2(g)                  CO(g) (b) Zn2+(aq) + H2S(g)               ZnS(s) + 2 H+(aq) (c) HCl(g) + H2O()                  H3O+(aq) + Cl–(aq) (d)H2(g) +  O2(g)                   H2O(g) 3.         Which of the following is more likely to precipitate the hydroxide ion? (a)...
At 2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g)...
At 2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g) + O2(g) If the initial concentration of NO is 0.120 M, what are the equilibrium concentrations of NO, N2, and O2? [O2]__?_____ M [N2]____?___ M [NO]___?____ M
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.
1: a) Write the equilibrium expression for the following: 2 NOCl (g) = 2 NO (g)...
1: a) Write the equilibrium expression for the following: 2 NOCl (g) = 2 NO (g) + Cl2 (g) b) In the reaction above, the equilibrium concentration of NOCl = [0.0610], NO=[0.0151], Cl2= [0.0142], what is the equilibrium constant? c) The initial concentration of NO2 in a closed container is 0.750 M. At equilibrium, the concentration of O2 is 0.125 M. What are the concentrations of NO2 and NO at equilibrium? 2 NO2 (aq) = 2 NO (aq) + O2...
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...
1- Given the equation (the arrow should be two directional), 2 SO2(g) + O2(g) ↔ 2...
1- Given the equation (the arrow should be two directional), 2 SO2(g) + O2(g) ↔ 2 SO3(g), if the activities of O2, SO3 and SO2 are respectively 0.019, 0.00019 and 0.01939, what is the value of K? A. 5200 B. 0.00020 C. none D. 5100 2-We can simplify an equilibrium position calculation from equilibrium constant by assuming the reactant concentration changes very little,so long as the change in reactant is _________ of the original concentration. A.=5% B.≤ 5% C.NONE D....
Two kmol of CO2 dissociate to form an equilibrium mixture of CO2, CO, and O2 in...
Two kmol of CO2 dissociate to form an equilibrium mixture of CO2, CO, and O2 in which 1.8 kmol of CO2 is present. For a pressure of 5 atm, determine the temperature of the equilibrium mixture, in K.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT