Answer:
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.
