A chemistry 11 question!!

I really need help a question from my Chem 11 worksheet....here is some background info first:
Okay this is the equation CaCl2(aq) + Na2CO3(aq) => CaCO3 + 2NaCl(aq)
there is 2.61696 g of Na2CO3 and 1.0854g of CaCl2......so the first part asked which of the reactants were excess ( I got Na2CO3) and the other question that I don't understand how to do is this:

Calculate the amount of calcium carbonate (CaCO3) that should theoretically form from the amount of the limiting reactant (which is CaCl2) ....please help answer this and if you need more information then just ask....:) cause I don't even understand what it's asking :$

all the question is asking is
1) determine the limiting reactant, which you did
2) using the amount of the limiting reactant, determine how much CaCO3 is produced, this is the theoretical yield.

CaCl2 + Na2CO3 --> CaCO3 + 2NaCl.....balanced
2.61696g Na2CO3 / 106g/mole = 0.0247moles Na2CO3

1.0854g CaCl2 / 110.9g/mole = 0.00979moles CaCl2

the molar ratio of CaCl2:Na2CO3 = 1:1, this means that 0.00979moles CaCl2 only requires 0.00979moles Na2CO3. therefore, CaCl2 is the limiting reactant since there is more than enough Na2CO3.

theoretical yield:
0.00979moles CaCl2 x (1CaCO3 / 1CaCl2) x 110.9g/mole = 1.0857g CaCO3 formed

you need to convert those numbers from grams to moles using the molecular weight of Na2CO3 and CaCl2

since CaCl2 is the limiting reactant, then you can only make as much product(CaCO3) as materials you have (CaCl2)... but you need to convert to moles of CaCl2 then you will have same number of moles of CaCO3