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

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

Explanation:

Given that

Size of boxes are equal

So volume of boxes = V

Temperature in box A = 50°C = 323 k

Temperature in box B = 10°C = 283 K

We know that for ideal gas

P V = m R T

The mass of gases is not given so we can not say that which have high temperature. Also be can not say that which box have more molecule.

We know that average kinetic energy is directly proportional to the absolute temperature of gas that is why we can say that box A will have more kinetic energy because it have high temperature. We know that is gas have high kinetic energy then we can say that it have high moving velocity.

So the option d and e is correct.

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