What is the volume (in m³)of a 0.25 mol of an unknown gas at a pressure of 545.3 mm Hg and 15 °C? A)8.1 × 10^-5 B)18.2 × 10^-3 C)4.3 × 10^-4 D)2.2 × 10^-1 E)1.2 × 10^-4

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Quizplus · Accepted Answer

To find the volume of the gas, 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 pressure from mm Hg to atm (1 atm = 760 mm Hg) and the temperature from Celsius to Kelvin (K = °C + 273.15). P = 545.3 mm Hg * (1 atm / 760 mm Hg) = 0.7175 atm, T = 15 °C + 273.15 = 288.15 K. Using R = 0.0821 L·atm/(mol·K), V = nRT/P = (0.25 mol)(0.0821 L·atm/(mol·K))(288.15 K) / 0.7175 atm ≈ 8.2 L, which is 8.2 × 10^-3 m^3 (since 1 L = 10^-3 m^3), matching choice B.

What Is the Volume (In M3)of a 0

What Is the Volume (In M³)of a 0