Question

Consider this reaction:3Ca(s)+2H3PO4(aq)=Ca3(PO4)2(s)+3H2(g)How many grams of calcium are required to produce 50.500 g of calcium phosphate (MW = 310.19g/mol) assuming an excess of Phosphoric acid?

Answer 1

19.6 grams

Step-by-step explanation

Given:

Mass of calcium phosphate produced = 50.500 g

Equation: 3Ca(s) + 2H3PO4(aq) ---> Ca3(PO4)2(s) + 3H2(g)

What to find:

The grams of calcium required to produce 50.500 g of calcium phosphate.

Step-by-step solution:

From the equation, 3 mol Ca produce 1 mol Ca3(PO4)2

1 mole Ca3(PO4)2 = 310.19 grams

1 mole Ca = 40.078 grams

This means, (3 x 40.078 g) = 120.234 g Ca produce 310.19 g Ca3(PO4)2

So x grams Ca will be required to produce 50.500 grams Ca3(PO4)2

x grams Ca will be equal

`\frac{50.500\text{ }g}{310.19\text{ }g}*120.234g\text{ }Ca=19.6\text{ }grams\text{ }Ca`

The grams of calcium required to produce 50.500 g of calcium phosphate = 19.6 grams