Final answer:
The density of Freon 12, CF₂Cl₂, at 30.0 °C and 0.954 atm is 4.68 g/L option (c). This is calculated using the Ideal Gas Law and the molar mass of Freon 12.
Step-by-step explanation:
To calculate the density of Freon 12, CF₂Cl₂, at 30.0 °C and 0.954 atm, we must use the Ideal Gas Law equation, which is PV = nRT. We can rearrange the formula to solve for n (the amount of substance in moles), which is n = PV/RT. Once we have the number of moles, we can then find the mass by multiplying the number of moles by the molar mass of Freon 12 and finally dividing the mass by the volume to get the density.
However, we need the molar mass of CF₂Cl₂ to continue, which can be calculated by adding the atomic masses of C (12.01 g/mol), F (19.00 g/mol for each of the two fluorine atoms), and Cl (35.45 g/mol for each of the two chlorine atoms), resulting in the molar mass of CF₂Cl₂ to be approximately 120.91 g/mol.
The constant R (the ideal gas constant) has several different values depending on the unit used. Since we need density in g/L, we will use R = 0.0821 L·atm/K·mol.
Additionally, we must convert temperature to Kelvin by adding 273.15 to the Celsius temperature, so we use T = 30.0 °C + 273.15 = 303.15 K. Inserting the values we have into the n = PV/RT equation gives us:
n = (0.954 atm × 1 L) / (0.0821 L·atm/K·mol × 303.15 K) = 0.0384 moles
The mass of Freon 12 can be calculated as:
Mass = n × Molar mass = 0.0384 moles × 120.91 g/mol = 4.647 g
Finally, the density of Freon 12 at 30.0 °C and 0.954 atm is:
Density = Mass / Volume = 4.647 g / 1 L = 4.647 g/L, which we can round to 4.68 g/L (option c).