How many milliliters of calcium, with a density of 1.55 g/mL, are needed to produce 98.5 grams of calcium hydroxide in the single-replacement reaction below? Show all steps of your calculation as well as the final answer. Ca + H2O → Ca (OH) 2 + H2

Question

Sonny Sanchez

Chemistry

31 August, 21:16

How many milliliters of calcium, with a density of 1.55 g/mL, are needed to produce 98.5 grams of calcium hydroxide in the single-replacement reaction below? Show all steps of your calculation as well as the final answer. Ca + H2O → Ca (OH) 2 + H2

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Yandel Patrick · Answer 1

Answer is: 34,35 mL.

Reaction: Ca + 2H₂O → Ca (OH) ₂ + H₂

m (Ca (OH) ₂) = 98,5g.

n (Ca (OH) ₂) = m:M = 98,5g:74g/mol = 1,33mol.

From reaction: n (Ca) : n (Ca (OH) ₂) = 1:1.

n (Ca) = n (Ca (OH) ₂) = 1,33mol.

m (Ca) = n (Ca) ·M (Ca) = 1,33mol·40g/mol = 53,24g.

d (Ca) = 1.55 g/mL.

V (Ca) = m (Ca) : d (Ca) = 53,24g : 1.55 g/mL = 34,35 mL.