Question

This problem involves a molecular compound so both empirical and molecular formulas are required. A compound compose of Carbon, Hydrogen, and bromine is analyzed. It is found to contain 0.3194 g of C, 0.05361 f of H, and 2.125 g of BR. What is the empirical formula of the compound? If the compound is known to have 12 H atoms in it, what is the molecular formula of the compound?

Answer 1

Answer:

empirical formula = CH2Br

molecular formula = C2H12Br2

Explanation:

1. Start with the number of grams of each element, given in the problem.
2. Convert the mass of each element to moles using the molar mass from the periodic table.
3. Divide each mole value by the smallest number of moles calculated.
4. Round to the nearest whole number. This is the mole ratio of the elements

In this problem:

Carbon: .3194/12.0107 = .0266

Hydrogen: .05361/1.0794 = .0532

Bromine: 2.125/79.904= .0266

Divide all three numbers by .0266 to get:

C = 1

H = 2.00

Br = 1