   Chapter 15.6, Problem 1.2ACP

Chapter
Section
Textbook Problem

Hydrogen is used in the Haber-Bosch process, and this is made from natural gas in a process called steam reforming.CH4(g) + H2O(g)→CO(g) + 3 H2(g)CO(g) + H2O(g) → CO2(g) + H2(g) a. Are the two reactions above endo- or exothermic? b. To obtain the H2 necessary to manufacture 15 billion kilograms of NH3 what mass of CH4 is required, and what mass of CO2 is produced as a by-product (assuming complete conversion of the CH4)?

(a)

Interpretation Introduction

Interpretation: The given reaction has to be identified for endothermic or exothermic.

Concept Introduction: Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

Exothermic when ΔH is negative and endothermic when ΔH is positive.

Explanation
• CH4+H2OCO+3H2

ΔrH0=(1molCO/molrxn)[ΔfH0CO](1molCH4/molrxn)[ΔfH0(CH4)](2molH2O/molrxn)[ΔfH0(H2O)]

ΔrH0=(1molCO/molrxn)[110.5](1molCH4/molrxn)[74.87kJ/mol](2molH2O/molrxn)[241.8kJ/mol]=206

(b)

Interpretation Introduction

Interpretation: The mass of CO2 that is produced as a by-product has to be identified.

Concept Introduction: Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

Exothermic when ΔH is negative and endothermic when ΔH is positive.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 