   Chapter 20, Problem 73AE

Chapter
Section
Textbook Problem

# 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

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) N−H 391 N−N 160 N≡N 941 O−H 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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