According to kinetic molecular theory, which of the following statements are true about the behavior of gases?

the particles of a gas are in constant, random motion.

gases consist of small particles that are separated from one another by empty space.

collisions between gas particles are elastic.

all of the above statements explain the behavior of gases.

All of the above statements explain the behavior of gases.

Explanation:

The kinetic molecular theory is a model that seeks to explain the behaviour of gases. The model upon which the gas laws are derived is based on five hypotheses:

The molecules of gases are in constant random motion, colliding with themselves and the wall of the container holding the moleculesThese molecules are small compared to the spaces that separate themAs the gas molecules collides with one another and the wall of the container, pressure is created within the container holding the gasThe collision of these gas molecules does not lead to loss of any energy. That is, the collision is elastic.The average kinetic energy of the gas molecules is directly proportional to the temperature (in Kelvin) of the gas

Hence, all the statements in the options are correct.

For cyclohexane compounds drawn in a chair conformation:   -axial bonds are vertical  -equatorial bonds are parallel to two bonds within the ring.  thus, as i assume the chair conformation is drawn:   -the x group is in an axial position, as are the five other vertical bonds.  -three axial bonds are on the top face of the ring  -the other three axial bonds are on the bottom face  the position of the second substituent on each ring carbon is equatorial.  gauche groups must be on an adjacent carbon such as carbon 6 and carbon 2, and also gauche groups are rotated by 60 degrees relative to each other.  drawing the newman projections for c1–c2 and c1–c6 aids in visualizing the groups that are gauche to the y group on c1.  click this link and watch some academic videos that may you more understand the topic