[Shoutx]

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)
= m/mm
= 0.99/159.56
=0.0062 mols

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
= (0.0025x183.7)
= 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

[Borek]

1, 2 are OK.

Are salts dissociated? If so, write them as ions.

What about products - dissociated? Not?