   Chapter 5, Problem 89GQ

Chapter
Section
Textbook Problem

Chloroform, CHCl3, is formed from methane and chlorine in the following reaction.CH4(g) + 3 Cl2(g) → 3 HCl(g) + CHCl3(g)Calculate ΔrH°, the enthalpy change for this reaction, using the enthalpies of formation of CO2(g), H2O(ℓ), CHCI3(g) (ΔfH° = –103.1 kJ/mol), and the enthalpy changes for the following reactions:CH4(g) + 2 O2(g) → 2 H2O(ℓ) + CO2(g)ΔrH° = –890.4 kJ/mol-rxn2 HCl(g) → H2(g) + Cl2(g)ΔrH° = +184.6 kJ/mol-rans

Interpretation Introduction

Interpretation:

The enthalpy change for the reaction of has to be calculated.

Concept Introduction:

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

ΔrH0 ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation

Given,

CH4+2O22H2O + CO2                                                ΔfH0-890.4kJ

Reverse the 2nd equation and multiply by 3.

3/2 H+ 3/2Cl23HCl                                                    ΔfH0-276.9kJ

Inorder to consume the CO2 formed in the 1st equation reverse the formation of CO2.

CO2C + O                                                                 ΔfH0-393.5kJ

In order to consume the H2O formed in the 1st equation reverse the formation of H2O

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