URGENT Chemistry Stoichiometry Help :S 1. The problem statement, all variables and given/known data Suppose that you use 1.110g of iron in this experiment. What is the minimum volume of 1.0M copper sulfate solution that you should add? 2. Relevant equations Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s) (1) 2Fe(s) + Cu2+(aq) --> 2Fe3+(aq) + 3Cu(s) (2) *****Since I do not know at this stage whether equation (1) or (2) is the appropriate one, I must base my calculation on whichever of the equations would require the most copper sulfate for a given quantity of iron***** 3. The attempt at a solution Here is what I believe to be a very poor attempt at solving the problem....any help will be greatly appreciated! 1.110g of Fe x (1 mol / 59.0 g Fe) = 0.018813559 moles Fe 0.018813559 mol Fe x (3 mol Cu2+ / 2 mol Fe) = 0.028220338 mol Cu2+ AND this is where I become stuck since the answer I need uses litres but all I have are the moles of Cu2+. Also, I don't know where the whole 1.0M from the question comes into play. I really need help. Thanks in advance!