If 5.05 g of Ca (OH) 2 and 6.70 g of H3PO4 are available, how many moles of Ca3 (Po4) 2 will you produce from each?

Question

Belinda Mcmahon

Chemistry

12 October, 17:57

If 5.05 g of Ca (OH) 2 and 6.70 g of H3PO4 are available, how many moles of Ca3 (Po4) 2 will you produce from each?

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Answers (1)

Know the Answer?

Anton Wilkerson · Answer 1

a) 0.023 mol Ca3 (PO4) 2 from 5.05 g Ca (OH) 2

b) 0.034 mol Ca3 (PO4) 2 from 6.70 g H3PO4

Explanation:

3Ca (OH) 2 + 2H3PO4 → Ca3 (PO4) 2 + 6H2O

∴ Mw Ca (OH) 2 = 74.093 g/mol

∴ Mw H3PO4 = 97.994 g/mol

a) n Ca3 (PO4) 2 = (5.05 g Ca (OH) 2) * (mol Ca (OH) 2/74.093 g) * (mol Ca3 (PO4) 2/3 mol Ca (OH) 2) = 0.023 mol Ca3 (PO4) 2

b) n Ca3 (PO4) 2 = (6.70 g H3PO4) * (mol H3PO4/97.994 g) * (mol Ca3 (PO4) 2/2 mol H3PO4) = 0.034 mol Ca3 (PO4) 2