Question

I am here to learn and understand. I am struggling on the following problem and would greatly appreciate some help to better understand. I will contribute and participate. I will upload the question once the thread becomes active.

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?

So this is a Percent Yield = Actual Yield/ Theoretical Yield x 100% problem. I'm just a little unsure about where to start?

Answer 2

Well first things first, is the equation balanced. 6CaO + P4O10 ---> 2Ca3(PO4)2. The answer is yes.

Answer 3

So again, we know the actual yield, right? 49.6 g Ca3(PO4)2. We need to find the theoretical yield before we can find the percent yield right? I become a little stumped right here. I'm not quite sure what to do next.

Answer 4

@sweetburger I don't mean to irritate you, but the way you explained the last problem was very helpful. I don't suppose you are talented in these types of problems as well? Sorry and thank you.

Answer 5

It states CaO is in excess therefore our limiting reactant in this problem is 28.4g of P4O10. Now we approach it searching for the theoretical yield in terms of grams of Ca3(PO4)2

Answer 6

now you just plug in the values for your answer into the percent yield equation.

Answer 7

I still following, just give me one more minute to look at your example. Thank you for taking the time.

Answer 8

No problem glad to help. I'm just working on some homework right now so take your time.

Answer 9

So when I'm looking at this I see some obvious cancellations. In the end it appears to all come down to multiplying and dividing, right? So would it look like this...?