The combustion of ethane in the presence of excess oxygen yields carbon dioxide and water:

2c2h6 (g) + 7o2 (g) → 4co2 (g) + 6h2o (l)

the value of δg° for this reaction is /mol. compare results for both methods of finding δg as done in class. is this difference significant?

ΔG° = - 2936.604 KJ/mol

Explanation:

⇒ ΔG°t = 4ΔG°fCO2(g) + 6ΔG°fH2O(l) - 7ΔG°fO2 - 2ΔG°fC2H6(g)

∴ ΔG°fCO2(g) = - 394.359 KJ/molfrom literature

∴ ΔG°fH2O(l) = - 237.178 KJ/mol

∴ ΔG°fO2(g) = 0.00 KJ/mol

∴ ΔG°fC2H6(g) = - 31.95 KJ/mol

⇒ ΔG°t = 4(- 394.359 KJ/mol) + 6(- 237.178 KJ/mol) - 7(0.00 KJ/mol) - 2( -31.95 KJ/mol)

⇒ ΔG°t = - 1577.436 KJ/mol - 1423.068 KJ/mol + 63.9 KJ/mol

⇒ ΔG°t  - 2936.604 KJ/mol

for points guys