What is the theoretical yield of ethyl chloride in the reaction of 19.2g g of ethylene with 48g g of hydrogen chloride?

This is a limiting reagent (LR) problem. I know that because amounts are given for BOTH reactants.

C2H4 + HCl ==> CH3CH2Cl

Convert grams C2H2 to mols. mols = grams/molar mass
Do the same for HCl

Using the coefficients in the balanced equation convert mols C2H4 to mols product.
Do the same for mols HCl to mol product.
It is likely these two values will not agree which means one of them is not right; the correct answer in LR problems is ALWAYS the smaller value and the reagent producing that value is the LR.

Now convert mols of the product to grams. mols = g x molar mass. This is the theoretical yield.

To determine the theoretical yield of ethyl chloride in this reaction, we need to use stoichiometry, which involves using the balanced equation and molar masses of the reactants and products.

First, let's write out the balanced equation for the reaction:

C2H4 (ethylene) + HCl (hydrogen chloride) -> C2H5Cl (ethyl chloride)

From the balanced equation, we can see that the molar ratio between ethylene and ethyl chloride is 1:1. This means that for every 1 mole of ethylene, we will produce 1 mole of ethyl chloride.

Next, we need to convert the given masses of ethylene and hydrogen chloride into moles. To do this, we divide each given mass by the molar mass of the respective compound.

The molar mass of ethylene (C2H4) can be calculated as follows:
(2 * molar mass of carbon) + (4 * molar mass of hydrogen) = (2 * 12.01 g/mol) + (4 * 1.01 g/mol) = 28.05 g/mol

Now we can calculate the number of moles of ethylene:
Number of moles = mass / molar mass = 19.2 g / 28.05 g/mol = 0.685 mol

Similarly, we calculate the number of moles of hydrogen chloride (HCl):
Molar mass of HCl = 1.01 g/mol + 35.45 g/mol = 36.46 g/mol
Number of moles = mass / molar mass = 48 g / 36.46 g/mol = 1.32 mol

Since the molar ratio between ethylene and ethyl chloride is 1:1, the number of moles of ethyl chloride produced will be equal to the number of moles of ethylene.

Therefore, the theoretical yield of ethyl chloride is 0.685 mol.

If you want to convert this value into grams, you can multiply the number of moles by the molar mass of ethyl chloride:

Molar mass of ethyl chloride (C2H5Cl) = (2 * molar mass of carbon) + (5 * molar mass of hydrogen) + molar mass of chlorine
= (2 * 12.01 g/mol) + (5 * 1.01 g/mol) + 35.45 g/mol = 64.52 g/mol

The mass of ethyl chloride will be:
Mass = number of moles * molar mass = 0.685 mol * 64.52 g/mol = 44.21 g

Therefore, the theoretical yield of ethyl chloride in this reaction is 44.21 grams.