What is the density of chlorine gas (g/L)at 1.01 atm and 54.1 °C?

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Quizplus · Accepted Answer

To find the density of chlorine gas at the given conditions, we can use the ideal gas law equation rearranged to solve for density ($\rho$):$\rho = \frac{PM}{RT}$Where:- $P$ is the pressure in atm (1.01 atm),- $M$ is the molar mass of chlorine gas (Cl2), which is approximately 70.9 g/mol (35.45 g/mol for Cl, times 2 because Cl2),- $R$ is the ideal gas constant, 0.0821 L·atm/(K·mol),- $T$ is the temperature in Kelvin. To convert 54.1 °C to Kelvin, we add 273.15, getting approximately 327.25 K.Plugging in the values:$\rho = \frac{(1.01 \, \text{atm})(70.9 \, \text{g/mol})}{(0.0821 \, \text{L·atm/K·mol})(327.25 \, \text{K})}$$\rho \approx 2.67 \, \text{g/L}$Therefore, the density of chlorine gas under the given conditions is approximately 2.67 g/L.

What Is the Density of Chlorine Gas (G/L)at 1