physics4u said:2.0 moles of nitrogen (N2) gas are placed in a container whose volume is 8.4e-3 m3. The pressure of the gas is 4.7e5 Pa. What is the average translational kinetic energy of a nitrogen molecule?
So I used PV=nRT and solved for T, after solving for Temperature, I used KE=3/2kT and solved for the total kinetic energy. Now is this my final answer or are there more steps to this problem?
physics4u said:2.0 moles of nitrogen (N2) gas are placed in a container whose volume is 8.4e-3 m3. The pressure of the gas is 4.7e5 Pa. What is the average translational kinetic energy of a nitrogen molecule?
So I used PV=nRT and solved for T, after solving for Temperature, I used KE=3/2kT and solved for the total kinetic energy. Now is this my final answer or are there more steps to this problem?
Shooting star said:For a diatomic gas, you should use 5/2 KT.
The average translational kinetic energy of a nitrogen molecule is approximately 5.92 x 10^-21 Joules at room temperature (25°C or 298 K).
The average translational kinetic energy of a nitrogen molecule can be calculated using the formula 1/2 * m * v^2, where m is the mass of the molecule and v is its average velocity.
The average translational kinetic energy of a nitrogen molecule can be affected by temperature, pressure, and the mass of the molecule. Higher temperatures and pressures will result in higher kinetic energy, while a heavier molecule will have a lower kinetic energy.
The average translational kinetic energy of a nitrogen molecule is important because it helps us understand the behavior and properties of gases. It is also a key factor in determining the temperature and pressure of a gas.
The average translational kinetic energy of a nitrogen molecule is similar to other diatomic molecules with similar masses, such as oxygen and hydrogen. However, it may differ from larger molecules or molecules with different shapes or structures.