Theoretical Yield Ni + 2HCl yields NiCl2 + H2
I have the balanced equation of Ni (s) + 2 HCl (aq) -> NiCl2 (aq) + H2 (g)
A.) If 12.0 moles of HCl were reacted, how many moles of Ni would be needed such that there was no excess?
B.) What is the theoretical yield (in grams) of NiCl2 from reacting 12.0 mol HCl?
C.) If 12.0 mol of HCl was reacted and the percent yield of the reaction was 78.5%, what was the actual yield (grams) of NiCl2?
I am completely lost when it comes to theoretical yield questions.. Any help is gladly needed! Thank-you!