Question

A 2.34-L gas sample in a cylinder with a freely moveable piston is initially at 24.0 ∘C. What is the volume of the gas when it is heated to 161 ∘C (at constant pressure)?

Answer 1

The volume of gas increases to approximately 3.43 L when it is heated from 24 degrees Celsius to 161 degrees Celsius at constant pressure according to Gay-Lussac's law.

Step-by-step explanation:

We can solve this problem using the Gay-Lussac's law. Gay-Lussac's law states that the pressure of an ideal gas is directly proportional to its absolute temperature when volume is held constant. But in this case volume can change, and since pressure remains constant, so we only focus on the volume and the temperature. We need to convert the temperatures from Celsius to Kelvin by adding 273 to each. So the initial temperature in Kelvin is 24 + 273 = 297 K and the final temperature is 161 + 273 = 434 K.

You can use the equation: V1 / T1 = V2 / T2 where V1 represents the initial volume (2.34 L), T1 the initial temperature (297 K), V2 the final volume, and T2 the final temperature (434 K). Plug in the known values into the equation and solve for V2 to find the final volume.

Our main answer comes out by cross multiplying and solving for V2 : V2 = V1 * T2 / T1 = 2.34 L * 434 K / 297 K The computation gives V2 approximately equal to 3.43 L.

Learn more about Gay-Lussac's law