Ok, so we have... Zn + CuCl2 -> ZnCL2 + Cu
And we are given that we have 28g of Zn (Zinc).
But the question calls for moles of ZnCl2.
So, the first step is to convert grams to moles of Zn.
We will need to find the AMU (Atomic Mass Units) that a Zn atom's mass.
A Zn atom has a mass of 63.546 AMU.
Now, we take the given mass and divide it by the mass of the atom to get the moles of reactant we have.
28g/63.546AMU≈ .4406257moles
If your teacher/ professor cares about sig figs, then it's .44 because you only have two sig figs from the given from the given mass of Zn (28g).
Now, the easy part.
What is the ratio of Zn atoms on the reactant side to Zn atoms on the product side?
1:1
And since we have excess CuCl2 Nothing else limits the reaction.
So, .44 (or how ever far your teacher wants you to round) moles of Zn reactants in a ideal environment (you will learn later that no reaction is 100% and that there are reactants always left over and how to solve for that) produces .44 moles of ZnCl2.
2HCl + Cu -> CuCl2 + H2 Assuming that it's Copper (II). CuCl2=Copper Chloride
CuCI2 does not exist, the correct formula is CuCl2 with a lowercase L. In water CuCl2 dissolves in watter tro produce Cu2+ and C- ions.
K[CuCl2]
Under normal conditions CuCl2 can exist in either a solid state or in aqueous solution.
no
2HCl + Cu -> CuCl2 + H2 Assuming that it's Copper (II). CuCl2=Copper Chloride
Cu and ZnCl2 are being produced.
CuCI2 does not exist, the correct formula is CuCl2 with a lowercase L. In water CuCl2 dissolves in watter tro produce Cu2+ and C- ions.
K[CuCl2]
CuCl2 is the product.
CuCl2
CuO + 2HCL - CuCl2 + H2O
cu(II) + 2agcl --> 2ag+cucl2
Under normal conditions CuCl2 can exist in either a solid state or in aqueous solution.
NiCl2 + 2Na --> 2NaCl + Ni
no
Cl