What is the average kinetic energy of a nitrogen molecule, N2 in the air for 100 degrees Fahrenheit?

To calculate the average kinetic energy of a nitrogen molecule, we can use the equation:

Average kinetic energy = (3/2) * (Boltzmann constant) * (temperature)

Where:
- The Boltzmann constant, denoted as "k," is a constant equal to 1.380649 x 10^-23 joules per kelvin (J/K).
- The temperature should be in kelvin (K).

To convert the temperature from Fahrenheit to Kelvin, we use the formula:

Temperature in Kelvin = (Temperature in Fahrenheit - 32) * (5/9) + 273.15

Let's calculate the average kinetic energy of a nitrogen molecule at 100 degrees Fahrenheit:

1. Convert the temperature from Fahrenheit to Kelvin:

Temperature in Kelvin = (100 - 32) * (5/9) + 273.15
= 37.778 * (5/9) + 273.15
= 310.928 Kelvin

2. Plug in the values into the average kinetic energy equation:

Average kinetic energy = (3/2) * (Boltzmann constant) * (temperature in Kelvin)
= (3/2) * (1.380649 x 10^-23 J/K) * (310.928 K)

Calculating the expression:

Average kinetic energy ≈ 6.2771 x 10^-21 J

Therefore, the average kinetic energy of a nitrogen molecule at 100 degrees Fahrenheit is approximately 6.2771 x 10^-21 joules.