Question

A gas undergoes a transformation at constant pressure, and the volume becomes 75 L. Knowing that the initial volume at 15 °C was 32 L, what is the temperature reached?

a) 273 °C
b) 48 °C
c) 0 °C
d) 33 °C

Answer 1

Using Charles's Law, the final temperature reached by the gas after expanding from 32 L at 15 °C to 75 L is calculated to be 402 °C at constant pressure.

Step-by-step explanation:

The subject of this question is Physics, specifically the topic of thermodynamics and gas laws. To find the temperature reached by the gas after its volume becomes 75 L when initially it was 32 L at 15 °C, we use Charles's Law. Charles's Law states that at constant pressure, the volume of a gas is directly proportional to its absolute temperature (in Kelvin).

To apply Charles's law, we convert the initial Celsius temperature to Kelvin (T1 = 15 + 273 = 288 K) and set up the proportion V1/T1 = V2/T2. Substituting the known values (V1 = 32 L, V2 = 75 L, T1 = 288 K), we can solve for the final temperature T2:

V1/T1 = V2/T2 →
32 L / 288 K = 75 L / T2 →
T2 = 75 L * 288 K / 32 L →
T2 = 675 K

Now, converting the final temperature back to Celsius, T2 = 675 K - 273 = 402 °C.

The temperature reached by the gas is 402 °C.