Which of the following is not correct about postulates of the kinetic molecular theory of gases?
1 . | Pressure of the gas is due to the collision of molecules against the walls of the container. |
2. | Volume of the gas is due to the large number of molecules of the gas. |
3. | Average kinetic energy of molecules is directly proportional to the absolute temperature of the gas. |
4. | The molecules move randomly with different speeds in different directions. |
A gas such as carbon monoxide would be most likely to obey the ideal gas law at?
1. High temperature and low pressure
2. Low temperature and high pressure
3. High temperature and high pressure
4. Low temperature and low pressure
If a gas expands at a constant temperature, it indicates that:
1. Kinetic energy of the molecules decreases
2. The pressure of the gas increases
3. The kinetic energy of the molecules remains the same
4. The number of molecules of gas increases
Average molar kinetic energy of CO and N2 at same temperature is:
1. KE1 = KE2
2. KE1 > KE2
3. KE1 < KE2
4. Can't say anything. Both volumes are not given.