Determine The Molecular Formula Of A Compound Whose Molecular Mass Is $60.00 \, \text{g/mol}$ And Has An Empirical Formula Of $CH_4N$.A. $CH_4N$ B. $C_2H_5N_2$ C. $C_2H_8N_2$ D. $C_3H_{12}N_3$
Introduction
In chemistry, determining the molecular formula of a compound is a crucial step in understanding its structure and properties. Given the molecular mass and empirical formula of a compound, we can use various techniques to determine its molecular formula. In this article, we will discuss how to determine the molecular formula of a compound with a molecular mass of 60.00 g/mol and an empirical formula of CH4N.
Understanding Empirical and Molecular Formulas
Before we dive into the calculation, let's understand the difference between empirical and molecular formulas. The empirical formula of a compound represents the simplest whole-number ratio of atoms of each element present in the compound. On the other hand, the molecular formula represents the actual number of atoms of each element present in a molecule of the compound.
Calculating the Molecular Formula
To calculate the molecular formula, we need to multiply the empirical formula by a factor (n) such that the molecular mass of the resulting formula is equal to the given molecular mass. The formula for calculating the molecular mass is:
Molecular Mass = (n × Empirical Formula Mass) + (n × Atomic Mass of each element)
where n is the multiplication factor.
Step 1: Calculate the Empirical Formula Mass
The empirical formula mass is the sum of the atomic masses of each element present in the empirical formula. The atomic masses of carbon (C), hydrogen (H), and nitrogen (N) are 12.01 g/mol, 1.008 g/mol, and 14.01 g/mol, respectively.
Empirical Formula Mass = (1 × 12.01) + (4 × 1.008) + (1 × 14.01) = 12.01 + 4.032 + 14.01 = 30.052 g/mol
Step 2: Calculate the Multiplication Factor (n)
We need to find the value of n such that the molecular mass of the resulting formula is equal to the given molecular mass of 60.00 g/mol. We can set up an equation using the formula:
Molecular Mass = (n × Empirical Formula Mass) + (n × Atomic Mass of each element)
60.00 = (n × 30.052) + (n × 12.01) + (n × 4.032) + (n × 14.01)
Simplifying the equation, we get:
60.00 = 30.052n + 12.01n + 4.032n + 14.01n 60.00 = 60.105n
Dividing both sides by 60.105, we get:
n = 60.00 / 60.105 = 1.00
Step 3: Calculate the Molecular Formula
Now that we have the value of n, we can calculate the molecular formula by multiplying the empirical formula by n.
Molecular Formula = n × Empirical Formula = 1 × CH4N = CH4N
However, this is the same as the empirical formula. This means that the molecular formula is the same as the empirical formula, and there is no need to multiply it by a factor.
Conclusion
In conclusion, the molecular formula of the compound with a molecular mass of 60.00 g/mol and an empirical formula of CH4N is CH4N. This is because the molecular mass of the empirical formula is already equal to the given molecular mass, and there is no need to multiply it by a factor.
Answer
The correct answer is A. CH4N.
Discussion
The molecular formula of a compound is a crucial piece of information that can help us understand its structure and properties. By using the empirical formula and molecular mass, we can determine the molecular formula of a compound. In this article, we discussed how to calculate the molecular formula of a compound with a molecular mass of 60.00 g/mol and an empirical formula of CH4N. We found that the molecular formula is the same as the empirical formula, and there is no need to multiply it by a factor.
References
- Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
- Chang, R. (2010). Chemistry: The central science. McGraw-Hill.
- Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.
Determining the Molecular Formula of a Compound: A Q&A Guide ===========================================================
Introduction
In our previous article, we discussed how to determine the molecular formula of a compound with a molecular mass of 60.00 g/mol and an empirical formula of CH4N. In this article, we will provide a Q&A guide to help you understand the concept of molecular formulas and how to calculate them.
Q: What is the difference between an empirical formula and a molecular formula?
A: The empirical formula of a compound represents the simplest whole-number ratio of atoms of each element present in the compound. On the other hand, the molecular formula represents the actual number of atoms of each element present in a molecule of the compound.
Q: How do I calculate the molecular formula of a compound?
A: To calculate the molecular formula, you need to multiply the empirical formula by a factor (n) such that the molecular mass of the resulting formula is equal to the given molecular mass. The formula for calculating the molecular mass is:
Molecular Mass = (n × Empirical Formula Mass) + (n × Atomic Mass of each element)
Q: What is the empirical formula mass?
A: The empirical formula mass is the sum of the atomic masses of each element present in the empirical formula. For example, if the empirical formula is CH4N, the empirical formula mass would be:
Empirical Formula Mass = (1 × 12.01) + (4 × 1.008) + (1 × 14.01) = 12.01 + 4.032 + 14.01 = 30.052 g/mol
Q: How do I calculate the multiplication factor (n)?
A: To calculate the multiplication factor (n), you need to set up an equation using the formula:
Molecular Mass = (n × Empirical Formula Mass) + (n × Atomic Mass of each element)
For example, if the molecular mass is 60.00 g/mol and the empirical formula mass is 30.052 g/mol, you can set up the equation as follows:
60.00 = (n × 30.052) + (n × 12.01) + (n × 4.032) + (n × 14.01)
Simplifying the equation, you get:
60.00 = 60.105n
Dividing both sides by 60.105, you get:
n = 60.00 / 60.105 = 1.00
Q: What if the molecular mass is not a whole number?
A: If the molecular mass is not a whole number, you may need to multiply the empirical formula by a fraction (n) rather than a whole number. For example, if the molecular mass is 60.50 g/mol, you can set up the equation as follows:
60.50 = (n × 30.052) + (n × 12.01) + (n × 4.032) + (n × 14.01)
Simplifying the equation, you get:
60.50 = 60.105n
Dividing both sides by 60.105, you get:
n = 60.50 / 60.105 = 1.005
Q: What if I get a negative value for n?
A: If you get a negative value for n, it means that the molecular mass is less than the empirical formula mass. This is not possible, so you should recheck your calculations.
Q: Can I use this method to calculate the molecular formula of any compound?
A: Yes, you can use this method to calculate the molecular formula of any compound, as long as you know the molecular mass and empirical formula.
Conclusion
In conclusion, determining the molecular formula of a compound is a crucial step in understanding its structure and properties. By using the empirical formula and molecular mass, you can calculate the molecular formula of a compound. We hope this Q&A guide has helped you understand the concept of molecular formulas and how to calculate them.
References
- Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
- Chang, R. (2010). Chemistry: The central science. McGraw-Hill.
- Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications. Pearson Prentice Hall.