Hi everyone, I'm having trouble with the following questions
Reaction: SrCl2+CuSO4 SrSO4 + CuCl2
25.0 mL of .1 molar strontium chloride and 0.99 g of copper.
Here are the Questions:
1) Determine which reactant is limiting and what mass of the other reactant should remain after the reaction is complete.
2) Determine the theoretical yield that was expected.
3) Write a net ionic equation for this reaction.
My Attempt at the question:
Moles of SrCl2 = 0.0025 (0.025X0.1)
Moles of Cu(SO4)
This would make SrCl2 the limiter in the reaction. Is that right?
SrSO4 is the solid that forms...
1 mol CuSO4 reacts to make 1 mol SrSO4
So the mols of excess reagent left over would be 0.0062-0.0025 = 0.0037
m = n x mm
= (0.0037 x 159.6)
= 0.59g of the excess left over.
Does that sound right?
2) 1 mol of SrCl2 reacts to make 1 mol SrSO4
0.0025 mol x
x= 0.0025 mol
m = n x mm
= 0.46 g of SrSO4
3) No idea how to make the net ionic equation
Sorry if my answers are a little unclear I'm not exactly sure if I'm doing the right thing. Thanks everyone
Also, If you need me to clarify anything just lemme know