The Empirical Formula For A Compound Is $CH_2$. If $n$ Is A Whole Number, Which Shows A Correct Relationship Between The Molecular Formula And The Empirical Formula?A. \[$\text{empirical Formula Mass} / \text{molecular Mass} =

Understanding the Empirical Formula

The empirical formula of a compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound. In the given problem, the empirical formula is $CH_2$. This means that the compound contains one carbon atom and two hydrogen atoms in the simplest ratio.

Understanding the Molecular Formula

The molecular formula of a compound is a representation of the actual number of atoms of each element present in the compound. It is a more detailed representation of the compound's composition compared to the empirical formula.

Relationship Between Empirical and Molecular Formula

To establish a correct relationship between the empirical formula and the molecular formula, we need to consider the concept of multiplication. The molecular formula can be obtained by multiplying the empirical formula by a whole number, which is denoted by $n$. This means that the molecular formula is $n$ times the empirical formula.

Correct Relationship

The correct relationship between the empirical formula and the molecular formula can be expressed as:

$$\text{molecular formula} = n \times \text{empirical formula}$$

where $n$ is a whole number.

Calculating the Molecular Formula

To calculate the molecular formula, we need to multiply the empirical formula by the whole number $n$. In this case, the empirical formula is $CH_2$, and we need to find the molecular formula.

Let's assume that the molecular formula is $C_xH_y$. We can write the following equation:

$$C_xH_y = n \times CH_2$$

Simplifying the equation, we get:

$$C_xH_y = CH_2n$$

This means that the molecular formula is $CH_2n$, where $n$ is a whole number.

Empirical Formula Mass and Molecular Mass

The empirical formula mass is the sum of the atomic masses of the atoms in the empirical formula. In this case, the empirical formula is $CH_2$, and the empirical formula mass is:

$$\text{empirical formula mass} = 12 + 2 \times 1 = 14$$

The molecular mass is the sum of the atomic masses of the atoms in the molecular formula. In this case, the molecular formula is $CH_2n$, and the molecular mass is:

$$\text{molecular mass} = 12 + 2 \times 1 \times n = 12 + 2n$$

Correct Relationship Between Empirical Formula Mass and Molecular Mass

The correct relationship between the empirical formula mass and the molecular mass can be expressed as:

$$\text{molecular mass} = n \times \text{empirical formula mass}$$

where $n$ is a whole number.

Substituting the values, we get:

$$12 + 2n = n \times 14$$

Simplifying the equation, we get:

$$12 + 2n = 14n$$

Subtracting $2n$ from both sides, we get:

$$12 = 12n$$

Dividing both sides by 12, we get:

$$n = 1$$

This means that the whole number $n$ is equal to 1.

Conclusion

In conclusion, the correct relationship between the empirical formula and the molecular formula is:

$$\text{molecular formula} = n \times \text{empirical formula}$$

where $n$ is a whole number. The empirical formula mass and the molecular mass are related by the equation:

$$\text{molecular mass} = n \times \text{empirical formula mass}$$

where $n$ is a whole number. In this case, the whole number $n$ is equal to 1.

References

• Chemistry: An Atoms First Approach, by Steven S. Zumdahl
• General Chemistry: Principles and Modern Applications, by Linus Pauling
  Empirical Formula and Molecular Formula Q&A =============================================

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: What is the molecular formula of a compound?

A: The molecular formula of a compound is a representation of the actual number of atoms of each element present in the compound.

Q: How are the empirical formula and molecular formula related?

A: The molecular formula can be obtained by multiplying the empirical formula by a whole number, which is denoted by $n$. This means that the molecular formula is $n$ times the empirical formula.

Q: What is the correct relationship between the empirical formula mass and the molecular mass?

A: The correct relationship between the empirical formula mass and the molecular mass is:

$$\text{molecular mass} = n \times \text{empirical formula mass}$$

where $n$ is a whole number.

Q: How do I calculate the molecular formula from the empirical formula?

A: To calculate the molecular formula, you need to multiply the empirical formula by the whole number $n$. In this case, the empirical formula is $CH_2$, and we need to find the molecular formula.

Let's assume that the molecular formula is $C_xH_y$. We can write the following equation:

$$C_xH_y = n \times CH_2$$

Simplifying the equation, we get:

$$C_xH_y = CH_2n$$

This means that the molecular formula is $CH_2n$, where $n$ is a whole number.

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

A: The empirical formula mass is the sum of the atomic masses of the atoms in the empirical formula. In this case, the empirical formula is $CH_2$, and the empirical formula mass is:

$$\text{empirical formula mass} = 12 + 2 \times 1 = 14$$

Q: What is the molecular mass of a compound?

A: The molecular mass is the sum of the atomic masses of the atoms in the molecular formula. In this case, the molecular formula is $CH_2n$, and the molecular mass is:

$$\text{molecular mass} = 12 + 2 \times 1 \times n = 12 + 2n$$

Q: How do I determine the whole number $n$?

A: To determine the whole number $n$, you need to use the relationship between the empirical formula mass and the molecular mass. The correct relationship is:

$$\text{molecular mass} = n \times \text{empirical formula mass}$$

where $n$ is a whole number.

Substituting the values, we get:

$$12 + 2n = n \times 14$$

Simplifying the equation, we get:

$$12 + 2n = 14n$$

Subtracting $2n$ from both sides, we get:

$$12 = 12n$$

Dividing both sides by 12, we get:

$$n = 1$$

This means that the whole number $n$ is equal to 1.

Q: What is the significance of the whole number $n$?

A: The whole number $n$ represents the multiplication factor between the empirical formula and the molecular formula. In this case, the whole number $n$ is equal to 1, which means that the molecular formula is the same as the empirical formula.

Q: Can you provide an example of a compound with an empirical formula of $CH_2$ and a molecular formula of $C_2H_4$?

A: Yes, an example of a compound with an empirical formula of $CH_2$ and a molecular formula of $C_2H_4$ is ethene (C2H4).

In this case, the empirical formula mass is 14, and the molecular mass is 28. The whole number $n$ is equal to 2, which means that the molecular formula is twice the empirical formula.

Conclusion

In conclusion, the empirical formula and molecular formula are related by the equation:

$$\text{molecular formula} = n \times \text{empirical formula}$$

where $n$ is a whole number. The empirical formula mass and the molecular mass are related by the equation:

$$\text{molecular mass} = n \times \text{empirical formula mass}$$

where $n$ is a whole number. In this case, the whole number $n$ is equal to 1.

References

• Chemistry: An Atoms First Approach, by Steven S. Zumdahl
• General Chemistry: Principles and Modern Applications, by Linus Pauling