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Q.

The heat of hydrogenation for 3-methylbutene and 2-pentene are -30 kcal/mol and -28 kcal,/mol respectively. The heats of combustion of 2-methylbutane and pentane are - 784 kcal/mol and -782 kcal,/mol respectively. All the values are given under standard conditions. Taking into account that combustion of both alkanes give the same products, what is ∆H (in kcal/mol) for the following reaction under same conditions ?

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a

0

b

-4

c

-2

d

2

answer is B.

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Detailed Solution

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ΔH1=−30kcal/mol, ΔH2=(−784+782)kcal/mol, ΔH3=28kcal/mol
⇒ΔH1+ΔH2+ΔH3=−4kcal/mol

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The heat of hydrogenation for 3-methylbutene and 2-pentene are -30 kcal/mol and -28 kcal,/mol respectively. The heats of combustion of 2-methylbutane and pentane are - 784 kcal/mol and -782 kcal,/mol respectively. All the values are given under standard conditions. Taking into account that combustion of both alkanes give the same products, what is ∆H (in kcal/mol) for the following reaction under same conditions ?