A sample of helium gas occupies 355mL at 23^$\circ$C. If the container the He is in is expanded to 1.50 L at constant pressure, what is the final temperature for the He at this new volume A) 1,250^$\circ$C B) 978^$\circ$C C) 70.1^$\circ$C D) 80.0^$\circ$C E) 1,520^$\circ$C

Question

Quizplus · Accepted Answer

First, we need to convert the initial temperature to Kelvin: 
23°C + 273.15 = 296.15 K.

Using the formula for Charles’s Law, V1/T1 = V2/T2, we can rearrange to solve for T2: 
T2 = (V2/T1)*V1

T2 = (1500 mL/355 mL)*296.15 K = 1249.04 K.

Finally, we convert back to Celsius: 
1249.04 K - 273.15 = 975.89°C ≈ 978°C.

Therefore, the answer is B.

A Sample of Helium Gas Occupies 355mL at 23 ∘\circ∘ C If the Container the He Is in Is Expanded

A Sample of Helium Gas Occupies 355mL at 23^$\circ$C If the Container the He Is in Is Expanded