posted by Josh on .
I have a problem that has been driving me crazy trying to solve, and I was wondering if someone could help. The problem is this: "Given the reaction: CuSO4 + 4 NH3 ----> Cu(NH3)4SO4, if 10 grams of CuSO4 reacts with 30 grams of NH3, what is the theoretical yield of Cu(NH3)4SO4, what is the limiting reactant, how many grams of the excess reactant is left over, and if the actual yield is 12.6 grams, what is the percent yield?" I don't know if it's hard or not, but I keep getting stuck after finding the theoretical yield (176.24?). Could someone help?
Post what you have done. Getting a theoretical yield of 176 grams out of 40 grams of reactants is visionary.
I add up the atomic masses and get the theoretical yield, it's finding the limiting reactant that is getting to me.
What I mean to say is I add up the atomic masses of CuSO4 + 4 NH3 and get the theoretical yield of 176.24. Or am I finding it wrong?
Let me help you on this...
To find the limiting reactant first of all.
-You have to first find the moles you have of each reactant.
- then go and find out how much of each reactant do you need to consume the other reactant
- then compare it to how much moles you do have of each and the one that needs more to consume than you have is the limiting reactant
I'll start with this and PLEASE post your work as I'm NOT going to do all the work =) (I'll check later)