Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100. cm³ at 95^$\circ$C, and 1,000. mmHg. A) 0.19 g/mol B) 35.3 g/mol C) 70.9 g/mol D) 137 g/mol E) 384 g/mol

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Quizplus · Accepted Answer

To find the molar mass of Freon-11 gas, we can use the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. First, we need to convert all units to the standard units for the ideal gas law: pressure in atmospheres (atm), volume in liters (L), and temperature in Kelvin (K).1. Convert temperature from Celsius to Kelvin: T = 95 + 273.15 = 368.15 K2. Convert pressure from mmHg to atm: P = 1000 mmHg * (1 atm / 760 mmHg) = 1.3158 atm3. Convert volume from cm^3 to L: V = 100 cm^3 * (1 L / 1000 cm^3) = 0.1 LNow, we can rearrange the ideal gas law to solve for n (number of moles): n = PV / RTUsing R = 0.0821 L·atm/(mol·K) (the ideal gas constant), we get:n = (1.3158 atm * 0.1 L) / (0.0821 L·atm/(mol·K) * 368.15 K) = 0.00434 molFinally, to find the molar mass, we divide the mass of the gas by the number of moles:Molar mass = mass / n = 0.597 g / 0.00434 mol = 137.6 g/molRounding to the nearest whole number gives us 137 g/mol, which matches option D.

Determine the Molar Mass of Freon-11 Gas If a Sample ∘\circ∘

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