A sample of an ideal gas has a volume of 750 L at 298 K and a pressure of 1.00 atm. What is the number of moles of gas present? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

• A. 0.032 mol
• B. 18.2 mol
• C. 30.6 mol
• D. 9.1 mol

Answer: (C)

Verified step by step guidance

1. Identify the known variables from the problem: volume \(V = 750\) L, temperature \(T = 298\) K, pressure \(P = 1.00\) atm, 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 \(n\) is the number of moles of gas.
3. Rearrange the Ideal Gas Law to solve for \(n\): \(n = \frac{P \times V}{R \times T}\).
4. Substitute the known values into the rearranged equation: \(n = \frac{1.00 \times 750}{0.0821 \times 298}\).
5. Perform the calculation to find the number of moles \(n\) (do not calculate the final value here, just set up the expression).