Question

A 1-L sample of CO initially at STP is heated to 546 K, and its volume is increased to 2 L. What effect do these changes have on the number of collisions of the molecules of the gas per unit area of the container wall? A) Increases B) Decreases C) Remains the same D) Cannot be determined

Answer 1

Increasing the temperature and doubling the volume of the CO sample from STP to 546 K and 2 L, respectively, results in a decrease in the frequency of collisions per unit area of the container wall.

Step-by-step explanation:

When a 1-L sample of CO at standard temperature and pressure (STP) is heated to 546 K and its volume is increased to 2 L, several gas laws come into play to determine the effect on molecule-wall collisions. According to Charles's law, increasing the temperature of a gas will increase its volume if the pressure is held constant, resulting in a decrease in the number of collisions per unit area. Additionally, Amontons's law (Gay-Lussac's law) implies that with an increase in temperature, the kinetic energy of gas particles also increases. However, since the volume is doubled, this means the particles have twice the space to move about, and therefore the frequency of collisions with the container walls per unit area will decrease. The combined effect of these changes is that the number of collisions of the molecules of the gas per unit area of the container wall decreases.