Acid rain is a growing worldwide environmental problem. Naturally, rainwater sho

Question

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 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 (posing a major threat to 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. Atmospheric SO2 has many sources, with volcanoes being the primary natural contributor. However, the burning of fossil fuel as the result of human industrialization has led to a significant increase in atmospheric SO2 levels. The number of moles n of SO2 released from a coal-burning power plant can be determined from the density , volume V, and the molar mass mm of SO2 gas given off by the power plant. Part A If a given power plant released SO2 gas with a volume V of 1200 m3 at a density of 2.86 kg/m3 at standard pressure and temperature, how many moles n of SO2 are released? The atomic weight of sulfur is 32.07 u and the atomic weight of oxygen is 16.00 u. Express your answer in moles to three significant figures. n = mol

Explanation / Answer

Volume of SO2 is V = 1200m3

density is = 2.86 kg/m3

So, mass m = (1200m3)(2.86 kg/m3) = 3432 kg = 3432000g

Now, atomic mas of SO2 is = (32.07 + 2X16) = 64.07u

Thus, 64.07g of SO2 is equivalent to 1 mol

So number of moles in 3432000g of SO2 are n = 3432000g/64.07g

or, n = 53566.4 mol

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