A sample of chlorine gas is confined in a 6.20 liter container at 202 torr and 27 ° C. How many grams of chlorine gas are present in the sample?
Molar Mass(Cl₂) = 70.90 g/mol

Question

A sample of chlorine gas is confined in a 6.20 liter container at 202 torr and 27 ° C. How many grams of chlorine gas are present in the sample? Molar Mass(Cl₂) = 70.90 g/mol

Quizplus · Accepted Answer

To find the mass of chlorine gas in the container, 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 in Kelvin. First, we convert all units to the standard units for the ideal gas law: pressure in atm, volume in liters, and temperature in Kelvin.1. Convert pressure from torr to atm: $202 \, \text{torr} \times \frac{1 \, \text{atm}}{760 \, \text{torr}} = 0.2658 \, \text{atm}$2. Convert temperature from Celsius to Kelvin: $27°C + 273.15 = 300.15 \, K$3. Use the ideal gas law to solve for n (number of moles): $PV = nRT$   - $R = 0.0821 \, \text{L atm mol}^{-1} \text{K}^{-1}$   - $n = \frac{PV}{RT} = \frac{(0.2658 \, \text{atm})(6.20 \, \text{L})}{(0.0821 \, \text{L atm mol}^{-1} \text{K}^{-1})(300.15 \, K)}$   - $n \approx 0.0669 \, \text{moles}$4. Convert moles to grams using the molar mass of $Cl_2$: $70.90 \, \text{g/mol}$   - $mass = n \times \text{molar mass} = 0.0669 \, \text{moles} \times 70.90 \, \text{g/mol}$   - $mass \approx 4.74 \, \text{g}$Therefore, the mass of chlorine gas in the container is approximately 4.74 grams.

A Sample of Chlorine Gas Is Confined in a 6