Stoichiometry

[moletin2011]

I have been trying to do this lab all night and would love some help thank you!!!
DATA-
Mass of filter paper-.21 g
Actual mass of cupric sulfate-12.5 g
Actual mass of iron powder-2.25 g
Mass of copper metal-3.22 g
Mass of beaker-67.83 g
QUESTIONS-
1. Write a balanced equation for the reaction between cupric sulfate and iron.
2. How many moles of copper metal were actually produced? (mass of copper metal= 67.83grams)
3. What is the actual number of moles that were reacted?
4. What is the theoretical yield of copper metal based on this experiment?
5. WHat is the limiting reactant? How much copper metal is actually produced?
6. What is the % yield of this reaction?

THANK YOU SO MUCH IN ADVANCE!

[kingchemist]

CuSO4 + Fe ---> Cu + FeSO4
1 mol     1 mol    1 mol

moles Cu = mass Cu/molar mass of Cu = 3.22/approx 64g. (67.83g is the mass of the container???)

Find moles CuSO4 by mass CuSO4/molar mass CuSO4
Find mole Fe by mass Fe/molar mass Fe

Use the molar ratio in the equation at the top to find which reactant is limiting and use this one to find the expected mass of Cu

% Yield = (actual mass Cu/expected mass Cu) x 100