A compound is found to contain 31.42 % sulfur, 31.35 % oxygen, and 37.23 % fluorine by weight. To answer the questions, enter the elements in the order presented above. 1. What is the empirical formula for this compound? 2. The molecular weight for this compound is 102.1 g/mol. What is the molecular formula for this compound?

Explanation:

To obtain the empirical and molecular formula of this compound from the percent composition of the elements, we follow the steps below;

Step 1: Divide the percentage composition by the atomic mass

Sulphur = 31.42 / 32 = 0.9819

Oxygen = 31.35 / 16 = 1.9594

Flourine = 37.23 / 19 = 1.9595

Step 2: Divide by the lowest number

Sulphur = 0.9819 / 0.9819 = 1

Oxygen = 1.9594 / 0.9819 ≈ 2

Flourine = 1.9595 / 0.9819 ≈ 2

This means the ratio of the elements is 1 : 2: 2

The empirical formular (simplest formular of a compound) of the compound is;

SO₂F₂

To obtain the molecular formular (Actual formular of a compound);

(SO₂F₂)n = 102.1

Inserting the atomic masses and solving for n;

(102)n = 102.1

n ≈ 1

The molecular formular is; (SO₂F₂)₁ = SO₂F₂

metric time was an attempt to create a standard unit of time based off of 10, but it never took off an is not included in the metric system (si)

the formula for the conversion of temperature from degree celsius to kelvin is:

the sample of water at is converted to kelvin temperature by using the above formula as:

on comparing the two samples of water at or we can say that at and at respectively. the difference between the temperatures of two samples of water is:

hence, one can say that the sample of water at is greater than the sample of water at by .