Question

Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...

Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C:

C2H6 (g) + O2 (g)  → CO2 (g) + H2O (l) (unbalanced)

ΔHf C2H6 (g) = -84.7 kJ/mol; S C2H6 (g) = 229.5 J/K⋅mol;
ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S CO2 (g) = 213.6 J/K⋅mol;
ΔHf H2O (l) = -285.8 kJ/mol; SH2O (l) = 69.9 J/K⋅mol;
SO2 (g) = 205.0 J/K⋅mol

Homework Answers

Answer #1

First, balance:

C2H6 (g) + O2 (g)  → CO2 (g) + H2O (l)

C2H6 (g) + 7/2O2 (g)  → 2CO2 (g) + 3H2O (l)

now, substitute data

dG = dH - T*dS

dH = Hprod - Hreact = [2CO2 (g) + 3H2O (l) ] -[C2H6 (g) + 7/2O2 (g) ] = (2*-393.5 + 3*-285.8) - (-84.7 + 7/2*0) = -1559.7

dS = Sprod - Sreact = [2CO2 (g) + 3H2O (l) ] -[C2H6 (g) + 7/2O2 (g) ] = (2*213.6 + 3*69.9) - (229.5 + 7/2*205) = -310.1

now..

dG = -1559.7 - 298*(-310.1/1000)

dG = -1467.2 kJ/mol (this is based per 1 mol of C2H6)

if whole reaction is needed:

2C2H6 (g) + 7 O2 (g)  → 4CO2 (g) + 6H2O (l)

GRXN = 2*dG = 2*-1467.2 = -2934.4kJ

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
Find the ΔH and ΔE for the reaction below: C2H6(g) + 7/2 O2(g) à 2 CO2(g)...
Find the ΔH and ΔE for the reaction below: C2H6(g) + 7/2 O2(g) à 2 CO2(g) + 3 H2O (l) given the following data: ΔHf C2H6 = -84.7 kJ/mol                  ΔHf CO2 = -393.5 kJ/mol ΔHf H2O = -286 kJ/mol
1- Calculate ΔG o for the following reaction at 25°C. You will have to look up...
1- Calculate ΔG o for the following reaction at 25°C. You will have to look up the thermodynamic data. 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) 2- A reaction will be spontaneous only at low temperatures if both ΔH and ΔS are negative. For a reaction in which ΔH = −320.1 kJ/mol and ΔS = −99.00 J/K ·mol,determine the temperature (in °C)below which the reaction is spontaneous.
When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00 atm, H2O (l)...
When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00 atm, H2O (l) and CO2 (g) are formed with the evolution of 50.33 kJ of energy. Substance ∆Hºf (kJ mol -1) Sº (J mol -1 K -1) H2O (l) - 285.8 69.95 CO2 (g) - 393.5 213.7 O2 (g) 0.0 205.0 C3H8 (g) ? 270.2 Calculate the molar enthalpy of combustion, ∆Hºcomb , of propane and the standard molar enthalpy of formation, ∆Hºf , of propane gas.
Given tha delta hydrogen = -393.5 kJ for the rxn.: C(s) +O2(g) -> CO2(g), and given...
Given tha delta hydrogen = -393.5 kJ for the rxn.: C(s) +O2(g) -> CO2(g), and given that delta Hydrogen = -285.8 kj for the rxn.: H2(g)+ 1/2O2(g) -> H2O(l), and given that delta hydrogen = -84.7 kJ for the rxn .: 3H2(g) +2C +2C(graphite) -> C2H6(g), calculate the dleta hydrogen for the rxn C2H6(g) + 3 1/2O2(g) -> 2CO2(g) + 3HO(l) Delta hydrogen = kJ
What is ΔGo (in kJ) at 464 K for the following reaction? PbO(g) + CO2(g) →...
What is ΔGo (in kJ) at 464 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol)
For the reaction:                                 2 C (s) + H2(g) →C2H2(g) a) Calculate the enthalp
For the reaction:                                 2 C (s) + H2(g) →C2H2(g) a) Calculate the enthalpy of reaction (DHrxn) from the following reactions: Reaction                                                             Δ Hrxn(kJ/mol)2 C2H2(g)+ 5 O2(g) → 4 CO2(g) + 2 H2O (l)              -2599.2 C (s) + O2(g) → CO2(g)                                            - 393.5 2 H2(g) + O2(g) → 2H2O (l)                                      -571.8 b) If the DS for the reaction is equal to 652 J/mol, and the reaction proceeds at 25°C, would you expect the reaction to be spontaneous?
Calculate the standard enthalpy of reaction for 2 C(graphite) + 3 H2(g) C2H6(g) Given the following...
Calculate the standard enthalpy of reaction for 2 C(graphite) + 3 H2(g) C2H6(g) Given the following standard enthalpy of combustion data, ∆H˚comb (C(graphite) = –393.5 kJ·mol–1 H2(g) + ½ O2(g) H2O(l) ∆H˚rxn = –285.8 kJ·mol–1 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(l) ∆H˚rxn = –3119.6 kJ·mol–1 (a) –84.6 kJ·mol–1 (b) 2440.2 kJ·mol–1 (c) –3799.0 kJ·mol–1 (d) –224.5 kJ·mol–1(e) not enough information provided
1. Given the values of ΔGfo given below in kJ/mol, calculate the value of ΔGo in...
1. Given the values of ΔGfo given below in kJ/mol, calculate the value of ΔGo in kJ for the combustion of 1 mole of methane to form carbon dioxide and gaseous water. ΔGfo (CH4(g)) = -48 ΔGfo (CO2(g)) = -395 ΔGfo (H2O(g)) = -236 2. Given the values of So given below in J/mol K and of ΔHfo given in kJ/mol, calculate the value of ΔGo in kJ for the combustion of 1 mole of ethane to form carbon dioxide...
Consider the reaction C2H5OH(l) ---> C2H6(g) + (1/2)O2(g). Enter ∆S in J K-1 mol1, all others...
Consider the reaction C2H5OH(l) ---> C2H6(g) + (1/2)O2(g). Enter ∆S in J K-1 mol1, all others in kJ/mol to two significant figures. (a) Calculate ∆H, ∆S, and ∆G at 25 C and 1 atm. (b) Estimate ∆U at 25 C and 1 atm. (c) Estimate ∆H at 500 C and 1 atm
Use standard free energies of formation to calculate ΔG∘ΔG∘ at 25 ∘C∘C for each of the...
Use standard free energies of formation to calculate ΔG∘ΔG∘ at 25 ∘C∘C for each of the following reactions. Substance ΔG∘f(kJ/mol)ΔGf∘(kJ/mol) H2O(g)H2O(g) −−228.6 H2O(l)H2O(l) −−237.1 NH3(g)NH3(g) −−16.4 NO(g)NO(g) 87.6 CO(g)CO(g) −−137.2 CO2(g)CO2(g) −−394.4 CH4(g)CH4(g) −−50.5 C2H2(g)C2H2(g) 209.9 C2H6(g)C2H6(g) −−32.0 Fe3O4(s)Fe3O4(s) −−1015.4 KClO3(s)KClO3(s) −−296.3 KCl(s)KCl(s) −−408.5 Part A C(s,graphite)+2H2(g)→CH4(g)C(s,graphite)+2H2(g)→CH4(g) Express your answer to one decimal place and include the appropriate units. Part B Fe3O4(s)+4H2(g)→3Fe(s)+4H2O(g)Fe3O4(s)+4H2(g)→3Fe(s)+4H2O(g) Express your answer to one decimal place and include the appropriate units. Part C N2(g)+O2(g)→2NO(g)N2(g)+O2(g)→2NO(g) Express your answer...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT