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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide.

2 C8H18() + 25 O2(g) → 16 CO2(g) + 18 H2O()

rH° = −10,922 kJ/mol-rxn

What is the enthalpy change if you burn 1.00 L of isooctane (d = 0.69 g/mL)?

Interpretation Introduction

Interpretation:

The enthalpy change in isooctane has to be determined.

Concept Introduction:

Standard enthalpy of the reaction,ΔrHo, is the change in enthalpy that happens when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.

Enthalpy of the reaction,ΔrH, is the change in enthalpy that happens when matter is transformed by a given chemical reaction

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 

Explanation

Given,

  ΔrHo=-10922kJ/mol 

  Mass=0.69g

Determine the no of moles of isooctane in 0.69g

  0.69g(1mol÷114.23g) =0.0060mol

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

  ΔrH=enthalpy change

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