In a laboratory experiment using the ideal gas law, which value is considered the universal gas constant (R) when pressure is measured in atmospheres and volume in liters?

• A. 0.0821 L·atm·mol^{-1}·K^{-1}
• B. 1.00 L·atm·mol^{-1}·K^{-1}
• C. 8.314 J·mol^{-1}·K^{-1}
• D. 22.4 L·mol^{-1}

Answer: (A)

Verified step by step guidance

1. Understand that the universal gas constant, denoted as \(R\), is a proportionality constant in the ideal gas law equation: \(\displaystyle PV = nRT\), where \(P\) is pressure, \(V\) is volume, \(n\) is the number of moles, and \(T\) is temperature in Kelvin.
2. Recognize that the value of \(R\) depends on the units used for pressure, volume, and temperature. Different unit systems require different numerical values for \(R\) to keep the equation consistent.
3. Since the problem specifies pressure in atmospheres (atm) and volume in liters (L), identify the value of \(R\) that matches these units. This value is commonly known and tabulated in chemistry references.
4. Recall that when pressure is in atm, volume in liters, amount in moles, and temperature in Kelvin, the universal gas constant \(R\) is \$0.0821\ \mathrm{L \cdot atm \cdot mol^{-1} \cdot K^{-1}}$.
5. Note that other values of \(R\) such as \$8.314\ \mathrm{J \cdot mol^{-1} \cdot K^{-1}}\( correspond to SI units (pressure in pascals, volume in cubic meters), and \)22.4\ \mathrm{L \cdot mol^{-1}}$ is the molar volume of an ideal gas at standard temperature and pressure, not the gas constant.