the diagrams below show two pure samples of gas in identical closed containers. each particle in sample a…

the diagrams below show two pure samples of gas in identical closed containers. each particle in sample a has less mass than each particle in sample b. all of the particles are moving at the same average speed. which sample has the higher temperature? sample a; its particles have the higher average kinetic energy sample b; its particles have the higher average kinetic energy neither; the particles have the same average kinetic energy

the diagrams below show two pure samples of gas in identical closed containers. each particle in sample a has less mass than each particle in sample b. all of the particles are moving at the same average speed. which sample has the higher temperature? sample a; its particles have the higher average kinetic energy sample b; its particles have the higher average kinetic energy neither; the particles have the same average kinetic energy

Answer

Explanation:

Step1: Recall kinetic - energy formula

The average kinetic energy of gas particles is given by $K_{avg}=\frac{3}{2}kT$ and also $K_{avg}=\frac{1}{2}mv^{2}$. Given that the average speed $v$ is the same for both samples, and $m_A<m_B$.

Step2: Compare kinetic energies

Using $K_{avg}=\frac{1}{2}mv^{2}$, since $v$ is constant and $m_A < m_B$, we have $K_{avg - A}<K_{avg - B}$.

Step3: Relate kinetic energy to temperature

Since $K_{avg}=\frac{3}{2}kT$, higher average kinetic energy means higher temperature. So sample B has a higher temperature because its particles have higher average kinetic energy.

Answer:

sample B; its particles have the higher average kinetic energy