1.018 g of Freon-113 gas is trapped in a 145 mL container at 760. mmHg and 50.0^$\circ$C. What is the molar mass of Freon-113 A) 21.7 g/mol B) 28.8 g/mol C) 46.1 g/mol D) 186 g/mol E) 245 g/mol

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Quizplus · Accepted Answer

To find the molar mass of Freon-113, we can use the ideal gas law equation rearranged to solve for molar mass (M): $M = \frac{mRT}{PV}$, where $m$ is the mass of the gas, $R$ is the ideal gas constant, $P$ is the pressure, $V$ is the volume, and $T$ is the temperature in Kelvin. First, convert all units to SI units: 50°F = 10°C = 283.15 K, 760 mmHg = 1 atm, and 145 mL = 0.145 L. Using $R = 0.0821 \frac{L \cdot atm}{mol \cdot K}$, we find $M = \frac{(1.018 g)(0.0821 \frac{L \cdot atm}{mol \cdot K})(283.15 K)}{(1 atm)(0.145 L)} \approx 186 g/mol$.

1018 G of Freon-113 Gas Is Trapped in a 145 ∘\circ∘

1018 G of Freon-113 Gas Is Trapped in a 145 $\circ$