a container with a specific volume “v” changes to “2v.” what happens to the average distance between gas…

a container with a specific volume “v” changes to “2v.” what happens to the average distance between gas molecules? assume that pressure and temperature of the gas remain constant.\ndecrease\nincrease\nexpand indefinitely\nthere is not enough information to tell.

a container with a specific volume “v” changes to “2v.” what happens to the average distance between gas molecules? assume that pressure and temperature of the gas remain constant.\ndecrease\nincrease\nexpand indefinitely\nthere is not enough information to tell.

Answer

Explanation:

Step1: Recall Avogadro's law

At constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of the gas (Avogadro's law $V = kn$, where $V$ is volume, $n$ is number of moles and $k$ is a constant). Here the number of moles is constant and volume doubles.

Step2: Consider gas - molecule distribution

When the volume of the container doubles while the number of gas molecules remains the same, the gas molecules have more space to spread out. So the average distance between them increases.

Answer:

Increase