A Compound Is Found To Contain $50.05 \%$ Sulfur And $49.95 \%$ Oxygen By Mass. What Is The Empirical Formula For This Compound?A. $SO$ B. $S_2O$ C. $SO_2$ D. $S_2O_3$

A Compound's Hidden Formula: Unveiling the Empirical Formula of a Sulfur-Oxygen Compound

In the realm of chemistry, understanding the composition of compounds is crucial for unraveling their properties and behavior. One of the fundamental concepts in this field is the empirical formula, which represents the simplest whole-number ratio of atoms of each element present in a compound. In this article, we will delve into the world of sulfur-oxygen compounds and uncover the empirical formula of a compound containing $50.05 \%$ sulfur and $49.95 \%$ oxygen by mass.

The Empirical Formula: A Definition

The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound. It is a fundamental concept in chemistry that helps us understand the composition of compounds and their properties. The empirical formula is usually expressed as a chemical formula, which consists of the symbols of the elements present in the compound, along with their respective subscripts.

Given Data

We are given a compound that contains $50.05 \%$ sulfur and $49.95 \%$ oxygen by mass. Our goal is to determine the empirical formula of this compound.

Step 1: Convert Mass Percentages to Grams

To begin, we need to convert the mass percentages of sulfur and oxygen to grams. Let's assume we have a $100 \text{ g}$ sample of the compound.

• Mass of sulfur = $50.05 \%$ of $100 \text{ g}$ = $50.05 \text{ g}$
• Mass of oxygen = $49.95 \%$ of $100 \text{ g}$ = $49.95 \text{ g}$

Step 2: Convert Grams to Moles

Next, we need to convert the grams of sulfur and oxygen to moles.

• Moles of sulfur = $\frac{50.05 \text{ g}}{32.07 \text{ g/mol}}$ = $1.56 \text{ mol}$
• Moles of oxygen = $\frac{49.95 \text{ g}}{16.00 \text{ g/mol}}$ = $3.12 \text{ mol}$

Step 3: Divide by the Smallest Number of Moles

To obtain the simplest whole-number ratio of atoms, we need to divide the number of moles of each element by the smallest number of moles.

• Moles of sulfur = $\frac{1.56 \text{ mol}}{1.56 \text{ mol}}$ = $1$
• Moles of oxygen = $\frac{3.12 \text{ mol}}{1.56 \text{ mol}}$ = $2$

Step 4: Write the Empirical Formula

Now that we have the simplest whole-number ratio of atoms, we can write the empirical formula of the compound.

• Empirical formula = $SO_2$

In this article, we have successfully determined the empirical formula of a sulfur-oxygen compound containing $50.05 \%$ sulfur and $49.95 \%$ oxygen by mass. The empirical formula of this compound is $SO_2$. This result demonstrates the importance of understanding the composition of compounds and their properties, which is a fundamental concept in chemistry.

The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound. It is a fundamental concept in chemistry that helps us understand the composition of compounds and their properties. In this article, we have used the given data to determine the empirical formula of a sulfur-oxygen compound. The result demonstrates the importance of understanding the composition of compounds and their properties, which is a fundamental concept in chemistry.

The empirical formula of the compound is $SO_2$.
A Compound's Hidden Formula: Unveiling the Empirical Formula of a Sulfur-Oxygen Compound

In our previous article, we delved into the world of sulfur-oxygen compounds and uncovered the empirical formula of a compound containing $50.05 \%$ sulfur and $49.95 \%$ oxygen by mass. The empirical formula of this compound is $SO_2$. In this article, we will address some of the frequently asked questions related to the empirical formula of a sulfur-oxygen compound.

Q: What is the empirical formula of a compound?

A: The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound.

Q: How do you determine the empirical formula of a compound?

A: To determine the empirical formula of a compound, you need to follow these steps:

1. Convert the mass percentages of each element to grams.
2. Convert the grams of each element to moles.
3. Divide the number of moles of each element by the smallest number of moles.
4. Write the empirical formula of the compound.

Q: What is the difference between the empirical formula and the molecular formula of a compound?

A: The empirical formula of a compound represents the simplest whole-number ratio of atoms of each element present in the compound, while the molecular formula represents the actual number of atoms of each element present in a molecule of the compound.

Q: How do you determine the molecular formula of a compound?

A: To determine the molecular formula of a compound, you need to know the molar mass of the compound and the empirical formula. You can then use the following formula to calculate the molecular formula:

Molecular formula = (Empirical formula) x (Molar mass / Empirical formula mass)

Q: What is the significance of the empirical formula of a compound?

A: The empirical formula of a compound is significant because it represents the simplest whole-number ratio of atoms of each element present in the compound. This information is useful in understanding the properties and behavior of the compound.

Q: Can you give an example of a compound with an empirical formula of $SO_2$?

A: Yes, an example of a compound with an empirical formula of $SO_2$ is sulfur dioxide (SO2).

Q: What are some common compounds with an empirical formula of $SO_2$?

A: Some common compounds with an empirical formula of $SO_2$ include sulfur dioxide (SO2), sulfur trioxide (SO3), and sulfuric acid (H2SO4).

In this article, we have addressed some of the frequently asked questions related to the empirical formula of a sulfur-oxygen compound. The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound. It is a fundamental concept in chemistry that helps us understand the composition of compounds and their properties.

The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound. It is a fundamental concept in chemistry that helps us understand the composition of compounds and their properties. In this article, we have used the given data to determine the empirical formula of a sulfur-oxygen compound. The result demonstrates the importance of understanding the composition of compounds and their properties, which is a fundamental concept in chemistry.

The empirical formula of a sulfur-oxygen compound is $SO_2$.