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Calculating moles using volume, density, molar mass, pressure and temperature

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Acid rain is a growing worldwide environmental problem. Naturally, rainwater should have a pH of not less than 5.5, but in the northeastern United States for example, the average pH of the rainwater is about 4.5. The increased acidity of the rain kills plants and animals in lakes and streams, causes increased weathering and decomposition of limestone in statues and on buildings (a major problem for Greek antiquities), and creates problems with the production of fruit and vegetable crops. The major chemical involved is sulfur dioxide, SO2, which combines with rainwater to form sulfuric acid. Although sulfur dioxide has many sources including volcanoes and metal smelting, the main source is believed to be the burning of fossil fuel. The number of moles, n, of sulfur dioxide released from a coal-burning power plant can be determined from the density, d; volume, V; and the molar mass, Mm, of sulfur dioxide gas given off by the power plant.

If a given power plant released sulfur dioxide gas with a volume, V, of 1200 m3 at a density, d, of 2.86 kg/m3 at standard pressure and temperature, how many moles of sulfur dioxide are released?

Express your answer in moles to three significant figures.

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Solution Summary

The solution explains in both narrative and calculations to arrive at the answer.

Solution Preview

This question is one of conversions. To find the moles of SO2 gas, you need to find the total mass. 1200 m3 * 2.86 Kg/m3 = 3432 ...

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