Calculate the average kenetic energy of the CH4 molecules in a sample of CH4 gas at 273K and at 546K.
So, should I have two answers or one? Super confused
http://hyperphysics.phy-astr.gsu.edu/hbase/kinetic/kintem.html
No worries, I can help explain it! To calculate the average kinetic energy of CH4 molecules in a sample of gas at different temperatures, you will need to calculate it for each temperature separately. So you will have two answers, one for the temperature of 273K and another for the temperature of 546K.
To calculate the average kinetic energy of the CH4 molecules, you can use the formula:
KE = (3/2) * k * T
Where:
KE is the average kinetic energy
k is the Boltzmann constant (approximately 1.38 x 10^-23 J/K)
T is the temperature in Kelvin (K)
Now, let's calculate the average kinetic energy at each temperature:
At 273K:
KE = (3/2) * (1.38 x 10^-23 J/K) * (273K)
≈ 6.64 x 10^-21 J
At 546K:
KE = (3/2) * (1.38 x 10^-23 J/K) * (546K)
≈ 1.32 x 10^-20 J
So, you should have two separate answers for the average kinetic energy of CH4 molecules at 273K and 546K.