Volume Occupied by 0.28g of Nitrogen Gas at NTP

In this article, we will delve into the calculation of the volume occupied by 0.28 grams of nitrogen gas at Normal Temperature and Pressure (NTP). We will explore the concept of the Ideal Gas Law and its application in determining the volume of gases at a specific temperature and pressure.

The Ideal Gas Law

The Ideal Gas Law is a fundamental principle in gas chemistry. It describes the behavior of an ideal gas in relation to pressure, volume, temperature, and the amount of substance. The equation for the Ideal Gas Law is as follows:

PV nRT

Where:

P Pressure (usually in Pascals, Pa) V Volume (usually in cubic meters, m3) n Number of moles of gas R Ideal gas constant (8.314 J/(mol·K)) T Temperature (usually in Kelvin, K)

Nitrogen Gas at NTP

Nitrogen gas (N?) forms a significant part of our atmosphere, making up about 78% of the air. At Normal Temperature and Pressure (NTP), which is defined as 20°C (293.15 K) and 1 atm (101,325 Pa), we can determine the volume occupied by a given mass of nitrogen gas.

Calculation of Volume

To understand the volume occupied by 0.28 grams of nitrogen gas, we need to follow these steps:

Step 1: Determine the number of moles of N?

The molar mass of nitrogen (N?) is 28 grams per mole (g/mol). Therefore, the number of moles in 0.28 grams of nitrogen gas can be calculated as:

n mass / molar mass 0.28 g / 28 g/mol 0.01 mol

Step 2: Apply the Ideal Gas Law

Using the Ideal Gas Law (PV nRT), we can calculate the volume occupied by 0.01 moles of nitrogen gas at NTP.

P 1 atm (101,325 Pa)
T 293.15 K
R 8.314 J/(mol·K)

First, convert the pressure from atm to Pa:

P 1 atm * 101,325 Pa/atm 101,325 Pa

Now, we can solve for V:

V (nRT) / P (0.01 mol * 8.314 J/(mol·K) * 293.15 K) / 101,325 Pa

V (2.437 J) / 101,325 Pa 0.00002406 m3

Converting cubic meters to liters (1 m3 1000 liters):

V 0.00002406 m3 * 1000 0.02406 liters

This is a very small volume, and it is interesting to compare it to the value mentioned in the question. The value provided in the question, 0.224 liters, seems to be a approximation given for 1 mole of gas at NTP, and it can be derived using the molar volume of an ideal gas at NTP which is 22.4 liters.

V 0.02406 liters ≈ 0.1/10 * 22.4 liters 0.224 liters.

Conclusion

Understanding the Ideal Gas Law and how it applies to real gases like nitrogen at NTP is essential for chemical and physical engineers, chemists, and anyone interested in understanding the behavior of gases. The volume of 0.28 grams of nitrogen gas at NTP is approximately 0.024 liters, which is very close to the 0.224 liters value given for 1 mole of gas.

References

WikiPedia: Ideal Gas Law Dynamic Periodic Table

Keywords

Normal Temperature and Pressure Ideal Gas Law Nitrogen Gas