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anonymous
 one year ago
How many grams of calcium phosphate can be produced when 78.5 grams of calcium hydroxide reacts with excess phosphoric acid? Unbalanced equation: H3PO4 + Ca(OH)2 → H2O + Ca3(PO4)2
So I balanced the equation as 2H3PO4 + 3Ca(OH)2 = 6H2O + Ca3(PO4)2 but now I am stuck
anonymous
 one year ago
How many grams of calcium phosphate can be produced when 78.5 grams of calcium hydroxide reacts with excess phosphoric acid? Unbalanced equation: H3PO4 + Ca(OH)2 → H2O + Ca3(PO4)2 So I balanced the equation as 2H3PO4 + 3Ca(OH)2 = 6H2O + Ca3(PO4)2 but now I am stuck

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Vocaloid
 one year ago
Best ResponseYou've already chosen the best response.1well, you start with 78.5 g of calcium hydroxide. our steps are: 1. convert 78.5g of calcium hydroxide to moles, using molar mass 2. divide moles of calcium hydroxide by 3, since it takes 3 moles of calcium hydroxide to produce 1 mole of calcium phosphate. this gives us the number of moles of calcium phosphate produced 3. multiply that by the molar mass of calcium phosphate to go from moles to grams

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0So 78.5 g Ca(OH)2 x 74.093 g/mol = 5816.3 mol Ca(OH)2 5816.3 mol / 3 = 1938.8 mol Calcium Phosphate 1938.8 mol x 310.17g/mol = 601,357.6 g Am I right?

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.2no u are incooorect. Actually the no of moles are equal to mass divided by the molar mass so no of moles of Ca(OH)2 would be 78.5g/74.0932gmol^1 I think u better correct ur answers from that point !

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.2Did u get where u went wrong ?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Okay thank you so 78.5g / 74.093 g/mol = 1.06 mol Ca(OH)2 1.06 mol / 3 = .353 mol Ca3(PO4)2 .353 mol x 310.17 g/mol = 109.49 g Is this correct now?

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.2Exactly ! U got it right! :)

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0YAY thank you so much can I ask you another one if you don't mind?

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.2Yeah post it as another question maybe ?
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