Chapter 20, Problem 40PS

### 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

# In 2005, global SO2 emission was estimated to be 12.83 Cg (gigagrams). According to the EPA, 71% of SO2 emissions into the atmosphere is from coal-fired power plants. How much coal (in metric tons) must have been burned to produce this much SO2, assuming that coal is 2.0% sulfur?

Interpretation Introduction

Interpretation: The amount of coal burnt to produce the given amount of SO2 has to 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

General unit conversion:

1Gg=1000ton

Explanation

The balanced equation for the combustion of coal (2% Sulphur) is given as:

Sâ€‰â€‰(s)â€‰â€‰â€‰â€‰+â€‰â€‰O2â€‰(g)â€‰â€‰â€‰â†’â€‰â€‰SO2â€‰(g)â€‰.

Given:

Amountâ€‰ofâ€‰SO2â€‰emissionâ€‰=â€‰12.83â€‰Gg

From the equation we can say that if 1 gram Sulphur react with 1 gram oxygen to form 2 gram Sulphur dioxide.

If 12.83â€‰GgSO2 is produced, then the amount of Sulphur will be half of it.

Amountâ€‰ofâ€‰sulphurâ€‰=â€‰12.832=â€‰6

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