Made an error when posting.. Put in 2.272 g instead of 2.727 g....
Ok, I've been stuck on this problem for a bit. Tried looking how to do it in the text book to no avail.
I'll Start by posting the reaction and what steps I took.
Trying to find a theoretical yield for NiCl2*6H2O + 3C2H8N2 --> Ni(C2H8N2)3 +6H2O Starting with 2.727grams of the NiCl2*6H2O and 9.23mL of 3C2H8N2 at a density of 0.950g/mL...
First step was to calculate the molar mass of both reactants and product that was isolated. The Ni(C2H8N2)3. For the NiCl2*6H2O I got a mass of 237.69 g. The 3C2H8N2 was a bit different as I only had a volume and density. 9.23mL at a 0.950 density. For the mass, I multiplied the density and volume to get 8.7685g.
from here, things get fuzzy but here are the steps I took so far...
Find moles of reactant A
2.727g NiCl2*6H2Ox 1 mole NiCl2*6H2O/237.68g NiCl2*6H20 =0.01147 moles NiCl2*6H20
Find moles of reactant B
8.769g 3C2H8N2 x 1 mole 3C2H8N2/63.098g 3C2H8N2 = 0.13897 mol 3C2H8N2
From here, I'm lost.
Please help. Thanks in advance!
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So, I attempted to find the limiting reactant....