We are asked what mass of H_{2}SO_{4} is produced by the annual operation of the refrigerator.

C(s) + O_{2}(g) → CO_{2}(g), ΔH_{rxn} = –393.5 kJ/mol

SO_{2 }+ H_{2}O + 1/2O_{2} → H_{2}SO_{4}

Molar mass H_{2}SO_{4} = 98.09 g/mol

Molar mass S = 32.07 g/mol

Molar mass C = 12.01 g/mol

A typical frostless refrigerator uses 655 kWh of energy per year in the form of electricity. Suppose that all of this electricity is generated at a power plant that burns coal containing 3.3% sulfur by mass and that all of the sulfur is emitted as SO_{2} when the coal is burned. If all of the SO_{2} goes on to react with rainwater to form H_{2}SO_{4}, what mass of H_{2}SO_{4} is produced by the annual operation of the refrigerator? (Hint: Assume that the remaining percentage of the coal is carbon and begin by calculating ΔH˚_{rxn} for the combustion of carbon.)

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