Using the ideal gas law, what is the temperature (in K) of 0.300 mole of neon gas in a 2.00 L vessel at 4.68 atm?

• A. 273 K
• B. 450 K
• C. 381 K
• D. 182 K

Answer: (C)

Verified step by step guidance

1. Identify the known variables from the problem: number of moles \(n = 0.300\) mol, volume \(V = 2.00\) L, pressure \(P = 4.68\) atm, and the gas constant \(R = 0.0821\) L·atm/(mol·K). The temperature \(T\) is the unknown we need to find.
2. Write down the ideal gas law equation: \(P \times V = n \times R \times T\).
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: \(T = \frac{4.68 \times 2.00}{0.300 \times 0.0821}\).
5. Perform the arithmetic to calculate \(T\) (temperature in Kelvin) using the substituted values.