Which statement can best be concluded from the ideal gas law? the product of pressure and volume of an ideal gas is proportional to the absolute temperature. all collisions between atoms or molecules are perfectly elastic and are not the result of any attractive forces. the temperature, pressure, and volume of a gas are all related. the behavior of a gas under real conditions does not obey the ideal gas law.

The correct answer to the question is- A) The product of pressure and volume of an ideal gas is proportional to the absolute temperature.

EXPLANATION:

Let the pressure, volume and temperature of an ideal gas are  denoted as P , V  and T respectively.

From Boyle's law, we know that volume of a given mass of a gas is inversely proportional to the pressure at constant temperature.

Mathematically it can be written as -

                           (1)     [at constant temperature]

From Charle's law, we know that volume of a given mass of a gas is directly proportional to the absolute temperature at constant pressure.

Mathematically it can be written as -

                           V ∝ T           (2)   [at constant pressure]

Combining equations 1 and 2, we get-

                         ⇒  [K is a proportionality constant]

                        ⇒  

                         ⇒     [ans]

Hence, the correct option is the first option.

one person pulls 90n one way and the other has 100n pulling the other way.

so the net force = 90 - 100 = -10n,

or the ans can be 10n if the picture shows -90n and 100n instead.