Question

The temperature of the ideal gas in the container is 300K, occupying a volume (V) of 1.27 m². If the temperature is decreased to 100K without adding or removing blocks from the lid, what would be the new volume of the gas?

(a) 0.423 m²
(b) 1.27 m²
(c) 3.81 m²
(d) 4.23 m²

Answer 1

The new volume of the ideal gas when the temperature is decreased from 300K to 100K at constant pressure is found using Charles's Law. The calculation gives a new volume of 0.423 m³, which is option (a).

Step-by-step explanation:

The question involves applying Charles's Law, which describes how gases tend to increase in volume when the temperature rises at constant pressure, and decrease in volume when the temperature drops, assuming the amount of gas remains the same. To find the new volume (V2) of the gas when the temperature decreases from 300K to 100K, we use the law in the form of the equation V1/T1 = V2/T2. Here, V1 is the initial volume (1.27 m³), T1 is the initial temperature (300K), and T2 is the final temperature (100K). Solving for V2 we get:

V2 = V1 * (T2/T1) = 1.27 m³ * (100K/300K) = 0.423 m³

Therefore, the new volume of the gas is 0.423 m³, which corresponds to option (a).