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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 19, Problem 73AE
Textbook Problem
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Hydrazine (N2H4) is used as a fuel in liquid-fueled rockets. When hydrazine reacts with oxygen gas, nitrogen gas and water vapor are produced. Write a balanced equation and use bond energies from Table 3-3 to estimate ∆H for this reaction.

Interpretation Introduction

Interpretation: The balanced equation for the reaction of hydrazine with oxygen is to be stated. The value of ΔH° for this reaction is to be calculated using the bond energies from Table 3-3 .

Concept introduction: The expression to calculate the value of ΔH° is,

ΔH°=npD°(bondsbroken)nrD°(bondsformed)

To determine: The balanced equation for the reaction of hydrazine with oxygen; the value of ΔH° for this reaction is to be calculated using the bond energies from Table 3-3 .

Explanation of Solution

The balanced reaction is,

N2H4(l)+O2(g)N2(g)+2H2O(g)

Reaction between hydrazine (N2H4) with oxygen (O2) yields nitrogen gas (N2) and water (H2O) . The balanced reaction is,

N2H4(l)+O2(g)N2(g)+2H2O(g)

The required value of ΔH° for the given reaction is 590kJ_ .

Refer to Table 3-3 .

The value of bond energy, D°(kJ/mol) , for the given reactant and product is,

Bonds D°(kJ/mol)
NH 391
NN 160
NN 941
OH 467
O=O 495

The formula of ΔH° is,

ΔH°=npD°(bondsbroken)nrD°(bondsformed)

Where,

  • np is the number of moles of each product

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Chapter 19 Solutions

Chemistry: An Atoms First Approach
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