Explanation The given reaction is CH 4 ( g ) + 2 O 2 ( g ) → CO 2 ( g ) + 2 H 2 O ( g ) The formula of energy change is Δ E = E r − E p (i) Where Δ E is change in energy E r is energy required to break the bond in the reactants E p is energy released when bonds form in product Bonds broken in reactant is CH 4 : 4 mol C − H H 2 O : 2 mol O − H Refer to table 3-3 Calculate broken bond energy of reactants CH 4 : 4 mol C − H = 413 kJ mol × 4 mol = 1652 kJ (ii) 2 mol O − O = 146 kJ mol × 2 mol = 292 kJ (iii) The formula of E r is E r = Energy of 4 mol C − H + Energy of 2 mol O − O (iv) Substitute the value of equation (ii) and (iii) in (iv) E r = Energy of 4 mol C − H + Energy of 2 mol O − O E r = 1652 kJ + 292 kJ E r = 1944 kJ Bonds f

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Chapter 8, Problem 72E

Interpretation Introduction

Interpretation: The change in energy ΔE is to be determined from bond energy values for the given reactions.

Concept introduction: The bond energy is the energy required to break apart a compound.

Energy change is defined as the sum of change in internal energy plus product of the system.

To determine: The value of energy change ΔE for the reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g)

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Chapter 8, Problem 71E

Chapter 8, Problem 73E

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Solution Summary: The author explains that the change in energy Delta E is determined from bond energy values for the given reactions.

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