Chapter 21, Problem 112GQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Using enthalpy of formation data in Appendix L, determine whether the decomposition of NH4NO3(s) to give N2O(g) and H2O(g) is endothermic or exothermic.

Interpretation Introduction

Interpretation:

To determine the reaction is endothermic or exothermic by using enthaply of formation.

Concept introduction:

Enthalpy of formation of the reaction can be calculated by following expression,

ΔrH°=nΔfH°(products)nΔfH°(reactants)

The standard enthalpy of formation is equals to sum of standard enthalpy of formation of products minus sum of standard enthalpy of reactants.

If the value of ΔrH is negative, then the reaction will be exothermic.

If the value of ΔrH is positive, then the reaction will be endothermic.

Explanation

The value of Î”rHâˆ˜ for the reaction is calculated below.

Given:

Refer to Appendix L for the values of standard entropies and enthalpies.

The standard enthalpy of NH4NO3(s) is âˆ’365.56Â kJ/mol.

The standard enthalpy of N2O(g) is 82.05Â kJ/mol

The standard enthalpy of H2O(g) is âˆ’241.83Â kJ/mol

The balanced chemical equation is:

â€‚Â NH4NO3(s)Â â†’N2O(g)Â +Â 2H2O(g)

The Î”rHo can be calculated by the following expression,

Î”rHÂ°=âˆ‘nÎ”fHÂ°(products)âˆ’âˆ‘nÎ”fHÂ°(reactants)=[[(1Â molÂ N2O(g)/mol-rxn)Î”fHÂ°[N2O(g)

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