What is the density of SF_6 gas (in g/L) at 1.00 atm and 25°C?

• A. 6.16 g/L
• B. 1.33 g/L
• C. 4.52 g/L
• D. 2.89 g/L

Answer: (A)

Verified step by step guidance

1. Identify the given conditions: pressure (P) = 1.00 atm, temperature (T) = 25°C, and the gas is sulfur hexafluoride (SF_6). Convert the temperature to Kelvin using the formula \(T(K) = T(°C) + 273.15\).
2. Recall the ideal gas law equation: \(PV = nRT\), where \(P\) is pressure, \(V\) is volume, \(n\) is moles of gas, \(R\) is the ideal gas constant, and \(T\) is temperature in Kelvin.
3. Rearrange the ideal gas law to find the molar volume \(V_m\) (volume per mole) at the given conditions: \(V_m = \frac{RT}{P}\).
4. Calculate the molar mass of SF_6 by adding the atomic masses of sulfur (S) and fluorine (F) atoms: \(M = M_S + 6 \times M_F\).
5. Use the formula for density \(\rho = \frac{mass}{volume} = \frac{molar\ mass}{molar\ volume} = \frac{M}{V_m}\) to find the density of SF_6 gas in g/L.