Calculate the volume of 12.0 g of helium at 54.5 °C and 1025 mm Hg.

Question

Quizplus · Accepted Answer

To calculate the volume of helium, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. First, convert the given conditions to the appropriate units: 54.5 °C = 327.65 K (since K = °C + 273.15), and 1025 mm Hg = 1.35 atm (since 1 atm = 760 mm Hg). The molar mass of helium is approximately 4.00 g/mol, so 12.0 g of helium is 3.00 moles (since n = mass/molar mass). The ideal gas constant R = 0.0821 L·atm/(mol·K). Plugging these values into the ideal gas law equation: V = nRT/P = (3.00 mol)(0.0821 L·atm/(mol·K))(327.65 K) / (1.35 atm) ≈ 59.8 L.

Calculate the Volume of 12