Response:
d) In container A, the average kinetic energy per molecule exceeds that of container B.
e) Molecules in A exhibit a higher speed than those in B.
Reasoning:
Both containers are of identical size.
This indicates that the volume of each container is equal to V.
Temperature in container A is 50°C, which equals 323 K.
Temperature in container B is 10°C, equating to 283 K.
According to the ideal gas law:
P V = m R T
The quantities of gas mass are unspecified, making it impossible to determine which has a higher temperature or a greater number of molecules.
However, it is known that the average kinetic energy is directly related to the absolute temperature of a gas; thus, the kinetic energy in container A is greater due to its higher temperature. A higher kinetic energy implies increased molecular velocity.
Consequently, options d and e are accurate.
d) In container A, the average kinetic energy per molecule exceeds that of container B.
e) Molecules in A exhibit a higher speed than those in B.
