Here is a worked example, Follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
http://www.jiskha.com/science/chemistry/stoichiometry.html
actual yield = theor yield x (%yield/100) = ??; otherwise, it can be done only by performing the experiment and measuring the actual yield.
First, we write the balanced chemical equation for the reaction between iron and copper (II) chloride:
Fe + CuCl2 → FeCl2 + Cu
From the balanced equation, we can see that 1 mole of iron reacts with 1 mole of copper (II) chloride to produce 1 mole of copper metal.
To find the molar mass of copper (II) chloride (CuCl2), we add the atomic masses of its constituent elements:
Atomic mass of Cu = 63.55 g/mol
Atomic mass of Cl = 35.45 g/mol (there are two chlorine atoms in CuCl2)
Molar mass of CuCl2 = 63.55 g/mol + 2 * 35.45 g/mol = 134.45 g/mol
Next, we calculate the number of moles of copper (II) chloride using its mass:
Number of moles = Mass / Molar mass
Number of moles = 34.0 g / 134.45 g/mol ≈ 0.253 mol
Since the reaction is stoichiometric, 0.253 moles of copper (II) chloride will react to produce the same number of moles of copper metal.
Finally, we calculate the mass of the copper metal produced using its molar mass:
Mass = Number of moles x Molar mass
Mass = 0.253 mol x 63.55 g/mol ≈ 16.1 g
Therefore, approximately 16.1 grams of copper metal would be produced when unlimited iron reacts with 34.0 grams of copper (II) chloride.