Question

Calculate enthalpy, entropy, gibbs energy at 498C and 6 bar for following reactions: Ch4 + H2O...

Calculate enthalpy, entropy, gibbs energy at 498C and 6 bar for following reactions:

Ch4 + H2O = CO + 3H2

CO + H2O = CO2 + H2

CH4 + 2H2O = CO2 + 4H2

Homework Answers

Answer #1

PFA.

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 steam reforming reaction can be described by the following two reactions: CH4 +H2O ↔ CO+3H2...
The steam reforming reaction can be described by the following two reactions: CH4 +H2O ↔ CO+3H2 CH4 +2H2O ↔ CO2 +4H2 Assume that both these reactions achieve equilibrium at 600 K. The equilibrium constants at this temperature for the two reactions are 0.41 and 1.09 respectively. Calculate the equilibrium composition if the starting composition is 5 moles of steam and 1 mole of methane at a pressure of 2 atm.
Calculate the enthalpy, entropy, gibbs energy, and internal energy of combustion of cyclohexane.
Calculate the enthalpy, entropy, gibbs energy, and internal energy of combustion of cyclohexane.
For which one of the following reactions will the enthalpy change be approximately equal to the...
For which one of the following reactions will the enthalpy change be approximately equal to the internal energy change ? 2 H2(g) + O2(g) → 2 H2O(ℓ) H2O(ℓ) → H2O(g) CaCO3(s) → CaO(s) + CO2(g) H2(g) + Br2(g) → 2 HBr(aq) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
Using the gibbs free energy equation (and the changes in enthalpy, entropy and gibbs free energy...
Using the gibbs free energy equation (and the changes in enthalpy, entropy and gibbs free energy that occur in the process) - use thermodynamics to describe why hydrophobic molecules spontaneously self-assemble into aqueous environments.
Which of the following processes/reactions have a negative entropy change? Which of the following processes/reactions have...
Which of the following processes/reactions have a negative entropy change? Which of the following processes/reactions have a negative entropy change? a) Sublimation of dry ice into CO2 gas b) Cs metal melting in your palm c) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) d) 2 CH4(g) → C2H2(g) + 3 H2(g)
So I had to calculate the Gibbs Free energy for all the reactions: Ca(s)+CO2(g)+12O2(g)→CaCO3(s) = ΔG∘...
So I had to calculate the Gibbs Free energy for all the reactions: Ca(s)+CO2(g)+12O2(g)→CaCO3(s) = ΔG∘ = -734  kJ   CaCO3(s)→CaO(s)+CO2(g) = 131  kJ CO(g)+H2O(g)→H2(g)+CO2(g) = -28.6 KJ but now I have to predict what lowering the temeprature will do to Gibbs Free Energy: it will decrease with decreasing temp. ΔG∘ will increase with decreasing temperature. ΔG∘ will change slightly with decreasing temperature.
Using average bond enthalpies, estimate the enthalpy change for the following reaction: CH4(g) + H2O(g)3H2(g) +...
Using average bond enthalpies, estimate the enthalpy change for the following reaction: CH4(g) + H2O(g)3H2(g) + CO(g) ____kJ
From the following data calculate the ΔHrxn for the following reaction: 2 C(s) + 2 H2O(g)...
From the following data calculate the ΔHrxn for the following reaction: 2 C(s) + 2 H2O(g)  CH4(g) + CO2(g) ΔHrxn = ________ Use the following reactions and given ΔH’s and show your work. CO(g) + H2(g) → C(s) + H2O(g) ΔHrxn = −131.3 kJ CO(g) + H2O(g) → CO2(g) + H2(g) ΔHrxn = −41.2 kJ CO(g) + 3 H2(g) → CH4(g) + H2O(g) ΔHrxn = −206.1 kJ
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration...
Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration of H2O is increased. (a) In which direction does the reaction shift to reestablish equilibrium? (b) What happens to the concentrations of CH4, CO2, and H2 as the reaction shifts to reestablish equilibrium?
Calculate Delta G for the following reactions: Rxn 1: CH4(g) + 2 O2(g) --> CO2(g) +...
Calculate Delta G for the following reactions: Rxn 1: CH4(g) + 2 O2(g) --> CO2(g) + 2 H2O(l) Rxn 2 2 H2 (g) + O2(g) --> 2 H2O(g)