One of these products contains 37.8% carbon by mass, 6.30% hydrogen by mass and55.9% chlorine by mass.Calculate the empirical formula of the product.Deduce the molecular formula of the product

To find the empirical formula, we first assume that we have 100g of the substance. This means that the percentages can be read directly as grams. So, we have:

37.8g of Carbon (C) 6.30g of Hydrogen (H) 55.9g of Chlorine (Cl)

Next, we convert these amounts into moles by dividing by the atomic mass of each element:

For Carbon: 37.8g / 12.01g/mol = 3.15 mol For Hydrogen: 6.30g / 1.01g/mol = 6.24 mol For Chlorine: 55.9g / 35.45g/mol = 1.58 mol

The empirical formula is the simplest, most reduced ratio of elements in a compound. To find this, we divide each of the mole quantities by the smallest quantity:

For Carbon: 3.15 mol / 1.58 mol = 2 For Hydrogen: 6.24 mol / 1.58 mol = 4 For Chlorine: 1.58 mol / 1.58 mol = 1

So, the empirical formula is C2H4Cl.

To find the molecular formula, we would need the molar mass of the compound, which is not provided in the question. If it were provided, we would divide it by the molar mass of the empirical formula to find the number of empirical formula units per molecule, and multiply the subscripts in the empirical formula accordingly.