A sample of an ideal gas has a pressure of 2.00 atm and a volume of 5.00 L at point A. If the amount of gas is 0.500 mol, what is the temperature of the gas (in kelvin) at point A? (R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 305 K
• B. 244 K
• C. 122 K
• D. 410 K

Answer: (A)

Verified step by step guidance

1. Identify the known variables from the problem: pressure \(P = 2.00\) atm, volume \(V = 5.00\) L, amount of gas \(n = 0.500\) mol, and the gas constant \(R = 0.0821\) L\cdot atm\cdot mol^{-1}\cdot K^{-1}$.
2. Recall the Ideal Gas Law equation: \(P \times V = n \times R \times T\), where \(T\) is the temperature in kelvin.
3. Rearrange the Ideal Gas Law to solve for temperature \(T\): \(T = \frac{P \times V}{n \times R}\).
4. Substitute the known values into the rearranged equation: \(T = \frac{2.00 \times 5.00}{0.500 \times 0.0821}\).
5. Calculate the value of \(T\) using the substituted numbers to find the temperature in kelvin.