Explanation Given information: Reactions- 2 H 2 ( g ) + O 2 ( g ) → 2 H 2 O ( g ) Δ H = − 483.6 kJ/mol 3 O 2 ( g ) → 2 O 3 ( g ) Δ H = 284.6 kJ/mol Reason for the correct option: The reaction with the unknown enthalpy change is given as follows: 3 H 2 ( g ) + O 3 ( g ) → 3 H 2 O ( g ) …… (1) The reactions with the known enthalpy changeis given as follows: 2 H 2 ( g ) + O 2 ( g ) → 2 H 2 O ( g ) Δ H = − 483.6 kJ/mol …… (2) 3 O 2 ( g ) → 2 O 3 ( g ) Δ H = 284.6 kJ/mol …… (3) Add three times of equation (2) and the reverse of equation (3) as follows: 3 [ 2 H 2 ( g ) + O 2 ( g ) → 2 H 2 O ( g ) ] Δ H = 3 ( − 483.6 ) kJ/mol 2 O 3 ( g ) → 3 O 2 ( g ) Δ H = − 284.6 kJ/mol Simplify the above equations to obtain enthalpy change of the required reaction, 6 H 2 ( g ) + 3 O 2 ( g ) → 6 H 2 O ( g ) Δ H = − 1450

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ISBN: 9780078021527

Author: Julia Burdge

Publisher: McGraw-Hill Education

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Chapter 5.5, Problem 1CP

Interpretation Introduction

Interpretation: The enthalpy change of the given reaction is to be calculated.

Concept introduction:

Hess’s law states that the change in enthalpy of a reaction remains same whether the reaction takes place in one step or in multiple steps. Enthalpy change is independent of path of the reaction

On adding the thermochemical equations, the value of enthalpy change is also added, which gives the enthalpy change of the net reaction.

On reversing any equation, the sign of the enthalpy change value is changed to the opposite sign.

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Solution Summary: The author explains that Hess's law states that the change in enthalpy of a reaction remains same whether the reaction takes place in one step or in multiple steps.

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