Consider the following data : Heat of formation of CO 2 ( g ) = − 393.5 kJ mol − 1 Heat of formation of H 2 O ( l ) = − 286.0 kJ mol − 1 Heat of combustion of benzene = − 3267.0 kJ mol − 1 The hea

Question

Consider the following data : Heat of formation of CO 2 ​ ( g ) = − 393.5 kJ mol − 1 Heat of formation of H 2 ​ O ( l ) = − 286.0 kJ mol − 1 Heat of combustion of benzene = − 3267.0 kJ mol − 1 The heat of formation of benzene is _ kJ mol − 1 . (Nearest integer)

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​ Δ H f ​ [ CO 2 ​ ( g ) ] = − 393.5 kJ / mole Δ H f ​ [ H 2 ​ O ( ℓ ) ] = − 286.0 kJ / mole Δ H c ​ [ C 6 ​ H 6 ​ ] = − 3267.0 kJ / mole Δ H f ​ C 6 ​ H 6 ​ = ( ?) C 6 ​ H 6 ​ + 2 15 ​ O 2 ​ ( g ) ⟶ 6 CO 2 ​ ( g ) + 3 H 2 ​ O ( ℓ ) Δ H R ​ = Δ H C ​ = ΣΔ H f ​ ( P ) − ΣΔ H f ​ ( R ) − 3267 = 6 × ( − 393.5 ) + 3 ( − 286 ) − Δ H f ​ ( C 6 ​ H 6 ​ ) Δ H f ​ ( C 6 ​ H 6 ​ ) = 48 kJ / mole ​

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