During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
(i) 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) ∆c H = –2658.0 kJ/mol
(ii) C4H10(g)
+ O2 (g) → 4CO2 (g) + 5H2O (g) ∆c H = –1329.0 kJ/mol
(iii) C4H10(g)
+ O2 (g) → 4CO2 (g) + 5H2O (l) ∆c H = –2658.0 kJ/mol
(iv) C4H10 (g)
+ O2 (g) → 4CO2 (g) + 5H2O (l) ∆c H = +2658.0 kJ/mol
During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
(i) 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) ∆c H = –2658.0 kJ/mol
(ii) C4H10(g) + O2 (g) → 4CO2 (g) + 5H2O (g) ∆c H = –1329.0 kJ/mol
(iii) C4H10(g) + O2 (g) → 4CO2 (g) + 5H2O (l) ∆c H = –2658.0 kJ/mol
(iv) C4H10 (g) + O2 (g) → 4CO2 (g) + 5H2O (l) ∆c H = +2658.0 kJ/mol
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1 Answer
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This is a Multiple Choice Questions as classified in NCERT Exemplar
option (iii)
Standard enthalpy of combustion is defined as the enthalpy change per mole (or per unit amount) of a substance when it undergoes combustion and all the reactants and products being in their standard states at the specified temperature.
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