Final answer:
To calculate the mass of Cr(OH)3 produced from 1.25 g of LiOH, convert the mass of LiOH to moles, determine the stoichiometric ratio from the balanced chemical equation, and then convert back to grams. The calculated mass of Cr(OH)3 is approximately 2.53 g, which doesn't match any of the provided answer choices.
Step-by-step explanation:
The first step to find out how many grams of Cr(OH)3 are produced from 1.25 g of LiOH is to balance the chemical equation. The balanced chemical equation is:
Cr(NO3)3(aq) + 3LiOH(aq) → LiNO3(aq) + Cr(OH)3(s).
We then convert the mass of LiOH to moles using its molar mass (Molar mass of LiOH = 23.95 g/mol).
moles of LiOH = mass of LiOH / molar mass of LiOH = 1.25 g / 23.95 g/mol ≈ 0.0522 mol.
From the balanced equation, 3 moles of LiOH produce 1 mole of Cr(OH)3. Therefore, the moles of Cr(OH)3 produced is 1/3 of the moles of LiOH:
moles of Cr(OH)3 = moles of LiOH / 3 = 0.0522 mol / 3 ≈ 0.0174 mol.
The molar mass of Cr(OH)3 is 145.3 g/mol. To find the mass of Cr(OH)3:
mass of Cr(OH)3 = moles of Cr(OH)3 × molar mass of Cr(OH)3 = 0.0174 mol × 145.3 g/mol ≈ 2.53 g.
Since none of the provided answer choices match the calculated value of 2.53 g, it seems there might be an error in the question or the answer choices given. Your instructor might need to be notified about this discrepancy.