What is the theoretical yield of ethyl chloride in the reaction of 20.2 of ethylene with 53 of hydrogen chloride? (For ethylene, 28 amu; for hydrogen chloride,36.5amu ; for ethyl chloride, 64.5 amu.) What is the percent yield if 23.5 of ethyl chloride is actually formed?

This is a limiting reagent problem. You don't have units listed.

To solve this problem, we need to determine the theoretical yield of ethyl chloride and then calculate the percent yield based on the actual yield.

1. Calculate the number of moles of each reactant:
- Moles of ethylene (C2H4) = mass / molar mass = 20.2 g / 28 g/mol
- Moles of hydrogen chloride (HCl) = mass / molar mass = 53 g / 36.5 g/mol

2. Write and balance the chemical equation for the reaction:
C2H4 + HCl → C2H5Cl

3. Find the limiting reactant:
Calculate the stoichiometric ratio of ethylene to hydrogen chloride using the coefficients of the balanced equation. The reactant with the smaller stoichiometric ratio is the limiting reactant, as it will be completely consumed.

- Ethylene (C2H4): 1 mole produces 1 mole of ethyl chloride
- Hydrogen chloride (HCl): 1 mole produces 1 mole of ethyl chloride

Therefore, both reactants have a 1:1 ratio, and neither is in excess.

4. Calculate the theoretical yield:
The theoretical yield is the maximum amount of product that can be obtained from the limiting reactant. Since both reactants are limiting, we can calculate the theoretical yield using either of them.

- Moles of ethylene (C2H4) = 20.2 g / 28 g/mol
- Moles of ethyl chloride (C2H5Cl) = Moles of ethylene (C2H4)
- Mass of ethyl chloride (C2H5Cl) = Moles of ethyl chloride (C2H5Cl) × molar mass = Moles of ethylene (C2H4) × molar mass(C2H5Cl)

5. Calculate the percent yield:
Percent yield = (Actual yield / Theoretical yield) × 100

- Actual yield of ethyl chloride = 23.5 g (given)
- Percent yield = (23.5 g / Theoretical yield) × 100

By following these steps, you should be able to determine the theoretical yield of ethyl chloride and calculate the percent yield.