According to the following reaction, how many grams of calcium sulfate will be formed upon the complete reaction of 30.1 grams of calcium hydroxide with excess sulfuric acid? sulfuric acid (aq) +calcium hydroxide (s)calcium sulfate (s) + water () grams calcium sulfate

55.32 g of CaSO₄.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

H₂SO₄ + Ca(OH)₂ —> CaSO₄ + 2H₂O

Next, we shall determine the mass of Ca(OH)₂ that reacted and the mass of CaSO₄ produced from the balanced equation. This can be obtained as follow:

Molar mass of Ca(OH)₂ = 40 + 2(16 + 1)

= 40 + 2(17)

= 40 + 34

= 74 g/mol

Mass of Ca(OH)₂ from the balanced equation = 1 × 74 = 74 g

Molar mass of CaSO₄ = 40 + 32 + (16×4)

= 40 + 32 + 64

= 136 g/mol

Mass of CaSO₄ from the balanced equation = 1 × 136 = 136 g

SUMMARY:

From the balanced equation above,

74 g of Ca(OH)₂ reacted to produce 136 g of CaSO₄.

Finally, we shall determine the mass of CaSO₄ produced by the reaction of 30.1 g of Ca(OH)₂. This can be obtained as follow:

From the balanced equation above,

74 g of Ca(OH)₂ reacted to produce 136 g of CaSO₄.

Therefore, 30.1 g of Ca(OH)₂ will react to produce = (30.1 × 136)/74 = 55.32 g of CaSO₄.

Thus, 55.32 g of CaSO₄ were obtained from the reaction.

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