Question

At some temperature, K = 16.3 for the following reaction: H2(g) + CO2(g) H2O(g) + CO(g)...

At some temperature, K = 16.3 for the following reaction: H2(g) + CO2(g) H2O(g) + CO(g) The initial partial pressures of H2 and CO2 are each 2.30 atm.

What is the final pressure of CO?

What is the final total pressure?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
For the reaction CO(g) + H2O(g) <=> CO2(g) + H2(g), Kp = 0.64 at 900 K....
For the reaction CO(g) + H2O(g) <=> CO2(g) + H2(g), Kp = 0.64 at 900 K. If the reaction is initiated with just H2(g) and CO2(g), each at a partial pressure of 0.540 atm, what is the partial pressure of CO(g) at equilibrium?
The equilibrium constant Kp for the reaction C(s)+H2O(g)?CO(g)+H2(g) is 2.44 at 1000 K. What are the...
The equilibrium constant Kp for the reaction C(s)+H2O(g)?CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO= 1.25 atm, and PH2= 1.60 atm? What is the equilibrium partial pressure of H2O? What is the equilibrium partial pressure of CO? What is the equilibrium partial pressure of H2?
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1326 torr and a H2O partial pressure of 1770 torr at 2000 K. A) Calculate the equilibrium partial pressure of CO2. B) Calculate the equilibrium partial pressure of H2.
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1344 torr and a H2O partial pressure of 1780 torr at 2000 K. calculate the equilibrium partial pressure of CO2. calculate the same for H2.
Consider the following equilibrium: CO2(g) + H2(g) CO(g) + H2O(g); Kc = 1.6 at 1260 K...
Consider the following equilibrium: CO2(g) + H2(g) CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose 0.038 mol CO2 and 0.022 mol H2 are placed in a 1.50-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/(K · mol)). The answer is either 9.9 atm or 1.1 atm when I solve using the quadratic equation but I can't decide which answer is correct.
Consider the following equilibrium: CO2(g) + H2(g) CO(g) + H2O(g); Kc = 1.6 at 1260 K...
Consider the following equilibrium: CO2(g) + H2(g) CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose 0.038 mol CO2 and 0.022 mol H2 are placed in a 1.50-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/(K · mol)). The answer is either 9.9 atm or 1.1 atm when I solve using the quadratic equation but I can't decide which answer is correct. Please explain how you eliminated the incorrect...
Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g) A) Find Kp for...
Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g) A) Find Kp for this reaction at 298 K B) What is 1) Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g). A) Find Kp for this reaction at 298 K. B) What is ΔH° for this reaction? C) What type of pressure and temperature change would favor CO production? D) What is K at 1000 K?
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.
At a certain temperature the reaction CO(g) + H2O(g) CO2(g) + H2(g) has Kc = 0.400....
At a certain temperature the reaction CO(g) + H2O(g) CO2(g) + H2(g) has Kc = 0.400. Exactly 1.00 mol of each gas was placed in a 100.0 L vessel and the mixture underwent reaction. What was the equilibrium concentration of each gas? [CO] = M [H2O] = M [H2] = M [CO2] =
1. Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.25 −L flask at a...
1. Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) A reaction mixture in a 5.25 −L flask at a certain temperature contains 26.8 g CO and 2.35 g H2. At equilibrium, the flask contains 8.64 g CH3OH. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. 2. Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1358 torr and a H2O partial pressure of 1764 torr at 2000 K....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT