Question

1. consider three identical flasks filled with different gases. flask a: co at 760 torr and 0°c flask b: n₂ at 250 torr and 0°c flask c: h₂ at 100 torr and 0°c a. in which flask will the molecules have the greatest average - kinetic energy? b. in which flask will the molecules have the greatest average velocity?

Explanation:

Step1: Recall the relationship between average kinetic energy and temperature

The average kinetic energy of gas molecules is given by the formula $\overline{KE}=\frac{3}{2}kT$, where $k$ is the Boltzmann constant and $T$ is the temperature in Kelvin. Since all flasks are at the same temperature ($T = 0^{\circ}C=273\ K$), the average kinetic energy of the molecules in each flask is the same.

Step2: Recall the relationship between average velocity and molar - mass

The average velocity of gas molecules is given by $\overline{v}=\sqrt{\frac{8RT}{\pi M}}$, where $R$ is the gas constant, $T$ is the temperature, and $M$ is the molar - mass of the gas. The molar - mass of $CO$ is $M_{CO}=(12 + 16)\ g/mol=28\ g/mol$, the molar - mass of $N_2$ is $M_{N_2}=(14\times2)\ g/mol = 28\ g/mol$, and the molar - mass of $H_2$ is $M_{H_2}=(1\times2)\ g/mol=2\ g/mol$. At the same temperature, the gas with the lowest molar - mass will have the greatest average velocity.

Answer:

a. The average kinetic energy is the same in all flasks (A, B, and C) since the temperature is the same in all of them.
b. Flask C ($H_2$) will have the molecules with the greatest average velocity because $H_2$ has the lowest molar - mass among the three gases at the same temperature.