Question

You have two flasks of equal volume. Flask A contains H2 at 0 °C and 1 atm pressure. Flask B contains CO2 gas at 25 °C and 2 atm pressure. Compare these two gases with respect to each of the following: (a) average kinetic energy per molecule (b) root mean square speed (c) number of molecules(d) mass of gas

Answer 1

The average kinetic energy per molecule is the same for both H2 and CO2. The root mean square speed of CO2 is higher due to its higher temperature. The number of molecules in each flask is equal, but the mass cannot be compared without additional information.

Step-by-step explanation:

To compare the gases H2 and CO2, we can analyze their properties:

1. Average kinetic energy per molecule: At a given temperature, the average kinetic energy of gas molecules is the same.
2. Therefore, the average kinetic energy per molecule in Flask A (H2) and Flask B (CO2) is equal.
3. Root mean square speed: The root mean square speed of a gas is directly proportional to the square root of the temperature. Given that the temperature of CO2 is higher, its root mean square speed will be higher as well.
4. Number of molecules: The number of molecules in a gas is directly proportional to its volume when the pressure and temperature remain constant.
5. Since the volume of both flasks is equal, the number of molecules in each flask will be the same.
6. Mass of gas: The mass of gas can be calculated using the ideal gas equation PV=nRT.
7. The mass of gas in each flask will depend on the number of moles (n) and the molar mass of the gas.
8. Without this information, we cannot compare the masses of the gases.