Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. Ca(OH)2 + H3PO4 --> Ca3(PO4)2 + H2OHow many grams of H3PO4 are needed to produce 1,460 grams of Ca3(PO4)2?Write your final answer in two decimal places.Use the following mass numbers:Ca - 40 g/molH - 1 g/molO - 16 g/molP - 31 g/mol
Question
Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. Ca(OH)2 + H3PO4 --> Ca3(PO4)2 + H2OHow many grams of H3PO4 are needed to produce 1,460 grams of Ca3(PO4)2?Write your final answer in two decimal places.Use the following mass numbers:Ca - 40 g/molH - 1 g/molO - 16 g/molP - 31 g/mol
Solution
First, we need to determine the molar mass of each compound involved in the reaction.
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Molar mass of Ca3(PO4)2: = 3*(40 g/mol for Ca) + 2*(31 g/mol for P) + 8*(16 g/mol for O) = 120 g/mol + 62 g/mol + 128 g/mol = 310 g/mol
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Molar mass of H3PO4: = 3*(1 g/mol for H) + 31 g/mol for P + 4*(16 g/mol for O) = 3 g/mol + 31 g/mol + 64 g/mol = 98 g/mol
Next, we need to determine the stoichiometry of the reaction. From the balanced chemical equation, we can see that 1 mole of H3PO4 reacts to produce 1 mole of Ca3(PO4)2.
Therefore, to find out how many grams of H3PO4 are needed to produce 1,460 grams of Ca3(PO4)2, we can use the following steps:
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Convert the mass of Ca3(PO4)2 to moles using its molar mass: = 1,460 g / 310 g/mol = 4.71 moles
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Since the stoichiometry of the reaction is 1:1, we need the same number of moles of H3PO4 to produce this amount of Ca3(PO4)2.
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Convert this amount in moles to grams using the molar mass of H3PO4: = 4.71 moles * 98 g/mol = 461.58 g
So, you would need approximately 461.58 grams of H3PO4 to produce 1,460 grams of Ca3(PO4)2.
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