Question

Debate continues on the practicality of H2 gas as a fuel. The equilibrium constant for the...

Debate continues on the practicality of H2 gas as a fuel. The equilibrium constant for the reaction CO(g)+ H2O (g) <--> CO2(g)+ H2 (g) is 1.0x10^5 at 25 degrees C. Calculate the standard free energy change (R=8.134 j/k*mol) and, without doing any calculations, estimate delta H(rxn) and delta S(rxn)

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
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 water–gas reaction, CO + H2O CO2 + H2 (a) Calculate the equilibrium constant, expressed...
Consider the water–gas reaction, CO + H2O CO2 + H2 (a) Calculate the equilibrium constant, expressed as log10 K, of the reaction at 298 K, (b) Calculate the equilibrium constant, expressed as log10 K, of the reaction at 1000 K
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 H2/CO ratio in mixtures of carbon monoxide and hydrogen (called synthesis gas) is increased by...
The H2/CO ratio in mixtures of carbon monoxide and hydrogen (called synthesis gas) is increased by the water-gas shift reaction CO(g)+H2O(g)⇌CO2(g)+H2(g), which has an equilibrium constant Kc= 4.24 at 800 K. Part A) Calculate the equilibrium concentration of CO if CO, H2O, CO2, and H2 are added to a reaction vessel with initial concentrations of 0.180 M. Express your answer to three decimal places and include the appropriate units. [CO]= Part B) Calculate the equilibrium concentration of H2O if CO,...
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the...
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. DELTA-H =___ kJ (c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? _____g (d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g)...
A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O...
A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(g)+H2(g)⇌CO(g)+H2O(g) Calculate Kc for the reaction.
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.
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] =
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?
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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT