Calculate the average kinetic energy of the N2 molecules in a sample of N2 gas at 266 K and at 532 K.
I got 32.7 and 65.5 but they're wrong??
K.E. = 3/2 k t
k = 1.38E-23
To calculate the average kinetic energy of N2 molecules, we can use the formula:
Average kinetic energy = (3/2) * R * T,
where R is the gas constant and T is the temperature in Kelvin.
First, we need to convert the temperatures given in degrees Celsius to Kelvin:
266 K = 266 + 273.15 = 539.15 K
532 K = 532 + 273.15 = 805.15 K
Now, we can calculate the average kinetic energy for each temperature:
For 266 K:
Average kinetic energy = (3/2) * R * T
= (3/2) * 8.314 J/(mol·K) * 539.15 K
≈ 32,771.8 J/mol
For 532 K:
Average kinetic energy = (3/2) * R * T
= (3/2) * 8.314 J/(mol·K) * 805.15 K
≈ 65,737.1 J/mol
Therefore, the correct average kinetic energies for the N2 molecules in a sample of N2 gas at 266 K and 532 K are approximately 32,771.8 J/mol and 65,737.1 J/mol, respectively.