Chapter 5, Problem 59PS

### 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

# The first step in the production of nitric acid from ammonia involves the oxidation of NH3.4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)(a) Use standard enthalpies of formation to calculate the standard enthalpy change for this reaction.(b) How much energy is evolved or absorbed as heat in the oxidation of 10.0 g of NH3?

(a)

Interpretation Introduction

Interpretation:

The standard enthalpy of reaction and heat evolved or absorbed is to be determined.

Concept Introduction:

The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.

Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation

Given,

â€‚Â Î”fH0(NH3)= -45.90kJ/mol

â€‚Â Î”fH0(NO)=-90.29kJ/mol

â€‚Â Î”fH0(H2O )-241.83kJ/mol

Î”rH0â€‰=â€‰[(4mol)(-90.29kj/mol)â€‰+â€‰(6mol)(-241

(b)

Interpretation Introduction

Interpretation:

The standard enthalpy of reaction and heat evolved or absorbed is to be determined.

Concept Introduction:

The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.

Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

The change in enthalpy, ΔH in kJ per mole of a given reactant for the reaction can be calculated as:

ΔrH=enthalpy changenumber of moles

ΔrH=ΔHnumber of moles

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