Question

the following reaction proceeds only 90% to completion: CO2(g) + H2O(g) ? H2(g) + CO2(g) The...

the following reaction proceeds only 90% to completion: CO2(g) + H2O(g) ? H2(g) + CO2(g) The carbon monoxide gas at 200°C and superheated steam at 600°C are fed into the process. The reaction proceeds 90% to completion. The pressure is maintained at 1atm throughout. The steam is added 200% in excess of that theoretically required for complete reaction. The final product mixture is ultimately removed from the system at 500°C. Using 1 mol of hydrogen produced as the basis of a. b. c. d. e. f. calculation, determine how much heat in KJ is absorbed or evolved in the process.

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

I hope you can understand the solution.

Thank YOU!!!

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
An isobaric reactor is fed an equimolar mixture of carbon monoxide (CO) and steam (H2O) at...
An isobaric reactor is fed an equimolar mixture of carbon monoxide (CO) and steam (H2O) at 400 K and 1 bar. If 60% of the H2O is converted to H2 through the following reaction, calculate how much heat must be added to the reactor in kJ/mol H2 produced if the product stream leaves the reactor at 700 K. Assume ideal gas behavior for all species. CO(g) + H2O(g) → CO2(g) + H2(g)
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] =
The reaction between carbon monoxide and water is given below: CO(g) + H2O(l) --------> CO2(g) +...
The reaction between carbon monoxide and water is given below: CO(g) + H2O(l) --------> CO2(g) + H2(g) We therefore know that which of the following reactions can also occur? a)  PbCl2(s) ---------->   Pb(s) + Cl2(g) b) CH4(g) + H2O(g) ----------> CO(g) + 3 H2(g) c) CO(g) + 3 H2(g) ------------------> CH4(g) + H2O(g) d) None of the Above
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]?
Consider the following reaction at equilibrium: C(s)+H2O(g)⇌CO(g)+H2(g) Predict whether the reaction will shift left, shift right,...
Consider the following reaction at equilibrium: C(s)+H2O(g)⇌CO(g)+H2(g) Predict whether the reaction will shift left, shift right, or remain unchanged upon each of the following disturbances. Part A C is added to the reaction mixture. -is added to the reaction mixture. -the reaction will shift left -the reaction will shift right -the reaction will remain unchanged Part B H2O is condensed and removed from the reaction mixture. -is condensed and removed from the reaction mixture. -the reaction will shift left -the...
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.
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 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.
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?
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=
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT