<span>I'm going to assume that the other reactant is sodium phosphate(you did not indicate this) so i'm guessing that the reaction did this CaCL2 + Na3(PO4) ------------> Ca3(PO4)2 + NaCl (since this reaction was done in water(aqueous solutions involved) the NaCl would be in the solution and thus the filtrate of the product so it won't influence the mass of the calcium phosphate product)
so then you need to write the balanced equation for this reaction(lets assume you can do this) 3 CaCL2 + 2 Na3(PO4) ------------> Ca3(PO4)2 + 6 NaCl
so in theoretical analysis 3 moles of calcium chloride is involved in the production of 1 mole of calcium phosphate
in terms of molar mass equivalents 3 molesw of calcium chloride weigh = 3 x (40 + 71)g/mol = 333g 1 mole of calcium phosphate = 310 g so if you only have 0.513 g of calcium chloride then this would calculate to get the mass of calcium phosphate mass = [0.513 / 333] x 310 g = 0.477grams
your actual yield is what you massed when you performed the lab. hope that helped. </span>
The major limitations of Newlands' law of octaves were : (i) It was applicable to only lighter elements having atomic masses upto 40 u, i.e., upto calcium. After calcium, the first and the eighth element did not have similar properties
