What does the kinetic theory state about the kinetic energy of gas molecules? a. the kinetic energy of gas molecules is inversely proportional to the kelvin temperature of the gas. b. the kinetic energy of gas molecules is directly proportional to the kelvin temperature of the gas. c. the kinetic energy of gas molecules is unaffected by the kelvin temperature of the gas. d. the kinetic energy of gas molecules is inversely proportional to the square of the kelvin temperature of the gas. reset next

option B. The kinetic energy of gas molecules is directly proportional to the Kelvin temperature of the gas.

Explanation:

The kinetic theory of gases explains the behavior and properties of gases from a molecular perspective.

Specifically and explicity, the kinetic theory of gases states that gases are constituted by particles (molecules) and that the average kinetic energy of the particles is proportional to the absolute temperature (Kelvin scale) of the gas. Furthermore, the temperature of all the (ideal) gases is the same at a given temperature.

Hence, you know that the higher the temperature of the gas, the higher the kinetic energy and the average speed of the molecules.

Other postulates of the kinetic theory of gases are that: i) the volume of the particles is neglectible; ii) the particles do not exhibit intermolecular attraction or repulsion; iii) the particles are in continuous random motion in straight paths, until they collide with other particles or the walls of the vessel, and iv) the collisions are elastic (the energy is conserved).

answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).