Four identical containers (1, 2, 3, and 4) each hold a different sample of gas at the same pressure. The number of moles of gas in each container is as follows: Container 1: 2 mol, Container 2: 1 mol, Container 3: 3 mol, Container 4: 0.5 mol. Which container has the gas stored at the highest temperature?

• A. Container 1
• B. Container 3
• C. Container 4
• D. Container 2

Answer: (B)

Verified step by step guidance

1. Recall the Ideal Gas Law, which relates pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T): \(P \times V = n \times R \times T\).
2. Since all containers are identical, they have the same volume (V), and the problem states that the pressure (P) is the same in all containers.
3. Rearrange the Ideal Gas Law to solve for temperature: \(T = \frac{P \times V}{n \times R}\).
4. Because P, V, and R are constant for all containers, temperature is inversely proportional to the number of moles: \(T \propto \frac{1}{n}\).
5. Compare the number of moles in each container; the container with the smallest number of moles will have the highest temperature.