Question

Calculate the mass of calcium sulfate that could be produced from 80g of calcium. Assume that the sulfuric acid is unlimited. Ca + H2SO4 -> CaSO4 + H2

A) 80g
B) 96g
C) 112g
D) 128g

Answer 1

The mass of calcium sulfate produced from 80g of calcium, assuming unlimited sulfuric acid, is calculated using the stoichiometry of the reaction
`\( \text{Ca} + \text{H}_2\text{SO}_4 \rightarrow \text{CaSO}_4 + \text{H}_2 \)`. The calculated mass is 271.61g, which does not match any of the given multiple-choice options.

Therefore, none of the given options (A) 80g, (B) 96g, (C) 112g, or (D) 128g are correct based on the stoichiometry of the given reaction.

Step-by-step explanation:

To calculate the mass of calcium sulfate that could be produced from 80g of calcium, we need to use stoichiometry. The balanced chemical equation is
`\( \text{Ca} + \text{H}_2\text{SO}_4 \rightarrow \text{CaSO}_4 + \text{H}_2 \)`. Each mole of calcium will react with one mole of sulfuric acid to produce one mole of calcium sulfate. We first need to calculate the number of moles of calcium used by using its molar mass (40.08 g/mol).

`\[\text{Number of moles of calcium} = \frac{\text{mass of calcium}}{\text{molar mass of Ca}} = \frac{80 \, \text{g}}{40.08 \, \text{g/mol}} = 1.996 \, \text{moles of Ca}.\]`

Using the stoichiometry of the reaction, 1 mole of calcium produces 1 mole of calcium sulfate. Hence, 1.996 moles of calcium would produce 1.996 moles of calcium sulfate. Now, we can calculate the mass of calcium sulfate produced by multiplying the number of moles of calcium sulfate by its molar mass (136.14 g/mol).

`\[\text{Mass of calcium sulfate} = \text{number of moles of CaSO}_4 * \text{molar mass of CaSO}_4 = 1.996 \, \text{moles} * 136.14 \, \text{g/mol} = 271.61 \, \text{g of CaSO}_4.\]`

Since the answer must match one of the multiple-choice options, it seems there may be an error in the available options as none match the calculated mass. Therefore, none of the given options (A) 80g, (B) 96g, (C) 112g, or (D) 128g are correct based on the stoichiometry of the given reaction.