We have two equal size boxes, A and B. Each box contains gas that behaves as an ideal gas. We insert a thermometer into each box

Question

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We have two equal size boxes, A and B. Each box contains gas that behaves as an ideal gas. We insert a thermometer into each box

and find that the gas in box S is at a temperature of 50°C while that in B is at 10°C. This is all we know about the gas in the boxes. Which of the following statements MUST be true? Which COULD be true? Explain the reasoning behind your answers.
a) The pressure in A is higher than in B
b) There are more molecules in A than in B
c) A and B cannot contain the same type of gas
d) The molecules in A have more average kinetic energy per molecule than those in B
e) The molecules in A are moving faster than those in B

Physics

1 answer:

Yuliya22 [3.3K] · Answer 1 · 2026-02-26T00:50:53+03:00

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.