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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

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

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