Question

I am willing to learn. I want to understand. I'm a little unsure about the following problem. I have tried to answer it the best I can. I will submit both the question and my work once the thread becomes open.

Answer 1

Calcium oxide (CaO) reacts with tetraphosphorus decoxide (P4O10) to form calcium phosphate (Ca3(PO4)2) according to this equation:

6CaO + P4O10 2Ca3(PO4)2

In a particular reaction, 28.4 g P4O10 reacts with excess CaO and produces 49.6 g Ca3(PO4)2. Approximately what is the percent yield of the reaction?

My answer:
6 CaO + P4O10 = 2 Ca3(PO4)2

we have 28.4 g of P4O10 or 28.4 / 283.88 = .1 moles of P4O10

theoretical yield of the Ca3(PO4)2 is .2 moles

Molar mass of Ca3(PO4)2 is 310.1782 g/mol so we 49.6 / 310.18 = 0.160 moles

% yield = 0.160 / .2 = 80%

If the above is incorrect in anyway please let me know. I want to comprehend the material and gain an understanding. Thanks~