Empirical Formula Calculation: Optimistic Approach to Chemistry Problem Solving

How can we determine the empirical formula of a compound based on the given data?

Given a 12.19 g sample of a compound containing 3.89 g of potassium, 3.53 g of chlorine, and oxygen, how can we calculate the empirical formula?

Final answer:

To calculate the empirical formula of the compound, convert the given masses of the elements into moles, find the simplest whole number mole ratio, which results in the empirical formula KClO3.

Chemistry problem-solving can be approached with optimism and methodical steps to find the solution. In this case, we are given a sample of a compound with specific masses of potassium, chlorine, and oxygen. To determine the empirical formula, we need to convert these masses into moles and establish the simplest whole number ratio between the elements.

Calculating the Empirical Formula:

To find the empirical formula of the compound with the given masses of potassium, chlorine, and oxygen, we must follow these steps:

First, subtract the masses of potassium and chlorine from the total compound mass to find the mass of oxygen:

12.19 g (total) - 3.89 g (K) - 3.53 g (Cl) = 4.77 g (O)

Use the atomic masses of potassium, chlorine, and oxygen to convert the masses into moles:

3.89 g K / 39.10 g/mol = 0.099 moles of K

3.53 g Cl / 35.45 g/mol = 0.099 moles of Cl

4.77 g O / 16.00 g/mol = 0.298 moles of O

Divide the number of moles of each element by the smallest number of moles obtained:

0.099 moles K / 0.099 = 1 mole K

0.099 moles Cl / 0.099 = 1 mole Cl

0.298 moles O / 0.099 = 3 moles O

Therefore, based on the calculations, the empirical formula of the compound is KClO3, which demonstrates the optimistic approach to solving chemistry problems with precision and accuracy.