Determine The Volume Of 50.0 G Of Nitrogen Dioxide At STP.

Mar 13, 2025 by ADMIN 59 views

**Determine the Volume of 50.0 g of Nitrogen Dioxide at STP**

Introduction

Nitrogen dioxide (NO2) is a toxic and highly reactive gas that plays a crucial role in various chemical reactions. Understanding the properties of NO2 is essential in various fields, including chemistry, environmental science, and engineering. In this article, we will discuss how to determine the volume of 50.0 g of nitrogen dioxide at standard temperature and pressure (STP).

What is Standard Temperature and Pressure (STP)?

STP is a set of standard conditions used to express the properties of gases. It is defined as a temperature of 0°C (273.15 K) and a pressure of 1 atm (101.325 kPa). These conditions are used as a reference point to compare the properties of different gases.

Molar Mass of Nitrogen Dioxide (NO2)

To determine the volume of NO2, we need to know its molar mass. The molar mass of NO2 is the sum of the atomic masses of nitrogen (N) and oxygen (O). The atomic mass of N is 14.01 g/mol, and the atomic mass of O is 16.00 g/mol. Therefore, the molar mass of NO2 is:

14.01 g/mol (N) + 2(16.00 g/mol) (O) = 46.01 g/mol

Determine the Number of Moles of NO2

To determine the volume of NO2, we need to know the number of moles of NO2 present. We can calculate the number of moles using the formula:

moles = mass / molar mass

Substituting the values, we get:

moles = 50.0 g / 46.01 g/mol = 1.088 mol

Determine the Volume of NO2 at STP

To determine the volume of NO2 at STP, we need to use the ideal gas law:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Rearranging the equation to solve for V, we get:

V = nRT / P

Substituting the values, we get:

V = (1.088 mol)(0.08206 L atm/mol K)(273.15 K) / (1 atm) = 24.51 L

Conclusion

In this article, we discussed how to determine the volume of 50.0 g of nitrogen dioxide at standard temperature and pressure (STP). We calculated the molar mass of NO2, determined the number of moles present, and used the ideal gas law to determine the volume of NO2 at STP. The volume of NO2 at STP is 24.51 L.

References

CRC Handbook of Chemistry and Physics, 97th Edition
International Union of Pure and Applied Chemistry (IUPAC)
National Institute of Standards and Technology (NIST)

Additional Information

Nitrogen dioxide (NO2) is a toxic and highly reactive gas that plays a crucial role in various chemical reactions.
The molar mass of NO2 is 46.01 g/mol.
The ideal gas law is a fundamental equation in chemistry that relates the pressure, volume, and temperature of a gas.
STP is a set of standard conditions used to express the properties of gases.

Frequently Asked Questions

Q: What is the molar mass of NO2? A: The molar mass of NO2 is 46.01 g/mol.
Q: How do I determine the number of moles of NO2? A: You can calculate the number of moles using the formula: moles = mass / molar mass.
Q: What is the volume of NO2 at STP? A: The volume of NO2 at STP is 24.51 L.

Q: What is the molar mass of NO2?

A: The molar mass of NO2 is 46.01 g/mol. This is the sum of the atomic masses of nitrogen (N) and oxygen (O).

Q: How do I determine the number of moles of NO2?

A: You can calculate the number of moles using the formula: moles = mass / molar mass. For example, if you have 50.0 g of NO2, you can calculate the number of moles as follows:

moles = 50.0 g / 46.01 g/mol = 1.088 mol

Q: What is the volume of NO2 at STP?

A: The volume of NO2 at STP is 24.51 L. This can be calculated using the ideal gas law: PV = nRT.

Q: What is the ideal gas law?

A: The ideal gas law is a fundamental equation in chemistry that relates the pressure, volume, and temperature of a gas. It is expressed as:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Q: How do I use the ideal gas law to determine the volume of a gas?

A: To use the ideal gas law to determine the volume of a gas, you need to know the pressure, number of moles, and temperature of the gas. You can then rearrange the equation to solve for V:

V = nRT / P

Q: What is STP?

A: STP is a set of standard conditions used to express the properties of gases. It is defined as a temperature of 0°C (273.15 K) and a pressure of 1 atm (101.325 kPa).

Q: Why is it important to know the volume of a gas at STP?

A: Knowing the volume of a gas at STP is important because it allows you to compare the properties of different gases under the same conditions. This is useful in various fields, including chemistry, environmental science, and engineering.

Q: Can I use the ideal gas law to determine the volume of a gas at other temperatures and pressures?

A: Yes, you can use the ideal gas law to determine the volume of a gas at other temperatures and pressures. However, you need to know the specific conditions of the gas, including the pressure, temperature, and number of moles.

Q: What are some common applications of the ideal gas law?

A: The ideal gas law has many common applications in chemistry, including:

Determining the volume of a gas at STP
Calculating the number of moles of a gas
Understanding the properties of gases under different conditions
Designing and optimizing chemical reactions and processes

Q: Can I use the ideal gas law to determine the volume of a gas that is not at STP?

A: Yes, you can use the ideal gas law to determine the volume of a gas that is not at STP. However, you need to know the specific conditions of the gas, including the pressure, temperature, and number of moles.

Q: What are some common mistakes to avoid when using the ideal gas law?

A: Some common mistakes to avoid when using the ideal gas law include:

Not knowing the specific conditions of the gas, including the pressure, temperature, and number of moles
Not using the correct units for the variables
Not checking the units of the gas constant (R)
Not considering the limitations of the ideal gas law, such as the assumption of ideal behavior and the neglect of intermolecular forces.