A coal source contains 1.1 % sulfur by mass. If 2.0 ×10^4 kg of coal is burned and forms oxides

step 1 Okay, so a coal source contains 1 .1 % sulfur by mass. And if we have 2 .04 times 10 to 4 kilogr

A coal source contains 1.1 % sulfur by mass. If 2.0 ×10^4...

A coal source contains $1.1 \%$ sulfur by mass. If $2.0 \times 10^{4} \mathrm{~kg}$ of coal is burned and forms oxides, calculate the mass of $\mathrm{CaSO}_{4}(s)$ that is produced from "scrubbing" the $\mathrm{SO}_{2}$ pollutant out of the exhaust gas. Assume that all of the sulfur in the coal is converted to calcium sulfate.

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Key Concepts

Molar Mass and Mole Conversion

Molar mass is the mass of one mole of a substance and provides the conversion factor between the mass of a substance and the amount in moles. This concept is vital for converting mass percentages into moles, facilitating the use of stoichiometric coefficients from balanced chemical equations to determine product yields.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in a chemical reaction using the relationships provided by a balanced chemical equation. It allows for the conversion of quantities from one substance to another based on mole ratios and is crucial in predicting the amounts of products formed under ideal reaction conditions.

Percent Composition

Percent composition is a way of expressing the proportion of a particular element in a compound or mixture as a percentage of its total mass. This concept is essential for determining how much of a specific element is present in a given mass of a material, which then allows one to calculate the mass of that element under various processing or reaction conditions.

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