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Which of the following statements are correct?

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For a reaction involving condensed phases $∆$ H = $∆$ U

It is possible to calculate the value of DH for the reaction $H_{2} (g) + B r_{2} (l) \to 2 H B r (g)$ from the bond enthalpy data alone.

The enthalpy of combustion of diamond and standard enthalpy of formation of carbon dioxide has the same value.

The reaction $N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$ is accompanied with decrease in entropy.

answer is A.

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Detailed Solution

A) For a reaction involving condensed phases (solids or liquids), $Δ v_{g}$ is zero.

B) Bond enthalpy data refers to gaseous species only.

C) Enthalpy of combustion of graphite and enthalpy of formation of carbon dioxide refer to one and the same chemical equation.

D) The reaction is accompanied with decrease in the gaseous species and, hence, decrease in entropy.

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