Question

For the reaction below, which of the following statements is(are) true? C2H5OH(l) + 3O2(g) →2CO2(g) + 3H2O(l) ΔH= –1.37 x 103 kJ/mol

I. The reaction is exothermic. II. The enthalpy change would be different if gaseous water were produced. III. The reaction is not an oxidation–reduction reaction.

Answer 1

C2H5OH(l) + 3O2(g) →2CO2(g) + 3H2O(l) ΔH= –1.37 x 103 kJ/mol

I. The reaction is exothermic = True

ΔH= –1.37 x 103 kJ/mol have negative therefore heat is evolved therefore reaction is exothermic

II. The enthalpy change would be different if gaseous water were produced = True

Enthalpy of formation of gases water = -241.8 KJ/mole

Enthalpy of formation of liquid water = -285.8 KJ/mole

therefore enthalpy change would be different if gaseous water were produced.

III. The reaction is not an oxidation–reduction reaction = False

in this reaction C in C2H5OH is get oxidized in CO₂ +4 oxidation state

and O₂ zero oxidation state get reduced to -2 oxidation in H₂O