Balanced equations:

- S(s) + O
_{2}(g) → SO_{2}(g) - SO
_{2}(g) + CaO (s) → CaSO_{3}(s)

$\mathbf{\%}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{S}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{S}\mathbf{}}{\mathbf{mass}\mathbf{}\mathbf{coal}}\mathbf{\times}\mathbf{100}$

$\mathbf{mass}\mathbf{}\mathbf{S}\mathbf{}\mathbf{=}\mathbf{1900}\mathbf{}\mathbf{tons}\mathbf{\times}\frac{\mathbf{2}\mathbf{.}\mathbf{5}}{\mathbf{100}}\mathbf{=}$**47.5 tons**

Mole to mole comparison:

- 1 mole of S produces SO
_{2} - 1 mole SO
_{2 }produces 1 mole CaSO_{3}

A particular coal contains 2.5% sulfur by mass. When this coal is burned, the sulfur is converted into sulfur dioxide gas. The sulfur dioxide reacts with solid calcium oxide to form solid calcium sulfite.

If the coal is burned in a power plant that uses 1900 tons of coal per day, how many grams of calcium sulfite are produced daily by this power plant? Express your answer using two significant figures.

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