   Chapter 20, Problem 32PS

Chapter
Section
Textbook Problem

One cubic meter of methane hydrate has 164 m3 of CH4 (at STP). If you burn the methane in 1.00 m3 of hydrate [to give CO2(g) and H2O(g)], how much energy, as heat, can be obtained?

Interpretation Introduction

Interpretation: The energy released by burning methane in 1.00m3 methane hydrate should be determined.

Concept introduction:

Enthalpy of combustion: At standard conditions when one mole of substance is burnt completely in presence of oxygen, the enthalpy change involved is called enthalpy of combustion.

ΔH0comb=nΔH0fproducts-nΔH0freactants

The number of moles from the volume is,

Numberofmoles=Volume at STP22.4L/mol

Explanation

When methane is burned, CO2 and H2O are produced as the products.

The balanced equation for the combustion of methane is given as:

CH4(g)+2O2(g)CO2(g)+2H2O(g).

Using the standard enthalpy of formation values, we can calculate the energy release when methane is burnt in the presence of oxygen.

Given:

ΔH0fof CO2=-393.509kJ/molΔH0fof H2O=-241.83kJ/molΔH0fofCH4=-74.87kJ/molΔH0fofO2=0kJ/mol

Change in enthalpy can be calculated by the equation:

ΔH0comb=nΔH0fproducts-nΔH0freactants

Substituting the values

ΔH0comb=[393

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

Find more solutions based on key concepts 