   Chapter 21, Problem 103GQ

Chapter
Section
Textbook Problem

The steering rockets in space vehicles use N2O4 and a derivative of hydrazine, 1,1 dimethyl hydrazine (Study Question 5.86). This mixture is called a hyperbolic fuel because it ignites when the reactants come into contact:H2NN(CH3)2(ℓ) + 2 N2O4(ℓ) → 3 N2(g) + 4 H2O(g) + 2 CO2(g)(a) Identify the oxidizing agent and the reducing agent in this reaction.(b) The same propulsion system was used by the Lunar Linder on moon missions in the 1970s. If the Linder used 4100 kg of H2NN(CH3)2, what mass (in kilograms) of N2O4 was required to react with it? What mass (in kilo-grams) of each of the reaction products was generated?

(a)

Interpretation Introduction

Interpretation:

To identify the oxidizing agent and reducing agent in the given reaction.

Concept introduction:

An oxidizing agent is a species which reduce other species by gaining electrons in a chemical reaction whereas a reducing agent is a species which loose electrons in the chemical reaction.

The oxidation number of an atom is the charge that atom would have if the compound was composed of ions or the total number of electrons that an atom gain or loss to form a chemical bond with another atom.

Explanation

The balanced chemical equation between NH2N(CH3)2 and N2O4 is written as,

NH2N(CH3)2(l)+2N2O4(l)3N2(g)+4H2O(g)+2CO2(g</

(b)

Interpretation Introduction

Interpretation:

To calculate the mass of N2O4 which is required to react with NH2N(CH3)2 and to calculate the mass of each product produced by the reaction of NH2N(CH3)2 with N2O4

Concept introduction:

Numberofmoles=MassMolecularmassMass=Numberofmoles×Molecularmass

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