Question

The diagram shows two samples of gas enclosed in identical containers. Each colored ball represents a gas particle. Both samples have the same number of particles.
Sample A
Mass of each particle: 28 u
Average particle speed: 980 m/s
Sample B
Mass of each particle: 44 u
Average particle speed: 1,100 m/s
Compare the average kinetic energies of the particles in each sample. Which sample has the
higher temperature?
Sample A
Sample B
Neither, both samples are the same.
ON

Answer 1

Answer:

Sample B

Explanation:

When heat is added to a substance, the molecules and atoms vibrate faster. Since the speed for Sample B is higher this means it has a higher temperature as well.

Answer 2

Answer:

The correct answer is Sample B.

Explanation:

The temperature of a system is directly related to the kinetic energy of the molecules. In the case of gases, as the temperature increases, the kinetic energy increases.

The formula of kinetic energy is:

$E_{k}$ = 1/2 * m * $v^{2}$

$E_{k}$: Kinetic energy of each particle.

m: Mass of each particle.

v: Speed of each particle.

For sample A:

$E_{kA}$ = $\frac{1}{2}$ * 28 * $980^{2}$

$E_{kA}$ = 13445600

For sample B:

$E_{kB}$ = $\frac{1}{2}$ * 44 * $1100^{2}$

$E_{kB}$ = 26620000

Being $E_{kB}$>$E_{kA}$, we can deduce that sample B has a higher temperature.

Have a nice day!