Chapter 20, Problem 32PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### 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:

â€‚Â CH4â€‰(g)â€‰â€‰â€‰â€‰+â€‰2â€‰O2â€‰(g)â€‰â€‰â€‰â†’â€‰â€‰â€‰â€‰â€‰CO2â€‰(g)â€‰+â€‰2â€‰H2Oâ€‰(g).

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

Given:

â€‚Â Î”H0fâ€‰ofÂ CO2â€‰â€‰=â€‰-393.509â€‰kJ/molÎ”H0fâ€‰ofÂ H2Oâ€‰â€‰=â€‰-241.83â€‰kJ/molÎ”H0fâ€‰ofâ€‰CH4â€‰â€‰â€‰=â€‰-74.87â€‰kJ/molÎ”H0fâ€‰ofâ€‰O2â€‰â€‰=â€‰0â€‰kJ/mol

Change in enthalpy can be calculated by the equation:

â€‚Â Î”H0combâ€‰â€‰â€‰=â€‰âˆ‘nâ€‰Î”H0fproductsâ€‰â€‰â€‰-âˆ‘nâ€‰Î”H0freactants

Substituting the values

â€‚Â Î”H0combâ€‰â€‰â€‰=â€‰[âˆ’393

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