Question

What is the density of freon-11 (cfcl3) at 120�c and 1.5 atm?

Answer 1

To calculate the density of freon-11 (CFCl3) at 120°C and 1.5 atm, you need to know its molar mass and use the ideal gas law equation. Convert the temperature to Kelvin, pressure to Pascal, and volume to liters. Substitute these values into the equation to calculate the mass, and then divide the mass by the volume to get the density.

Step-by-step explanation:

The density of a substance is defined as its mass per unit volume. To calculate the density of freon-11 (CFCl3), we need to know its molar mass and the ideal gas law equation.

The molar mass of CFCl3 is 137.37 g/mol. Using the ideal gas law equation, PV = nRT, we can rearrange it to find the mass using the equation m = (M * P * V) / (R * T), where M is the molar mass, P is the pressure, V is the volume, R is the ideal gas constant (0.0821 L * atm/(mol * K)), and T is the temperature in Kelvin.

Converting the temperature from Celsius to Kelvin (120°C + 273.15 = 393.15 K), the pressure from atm to Pascal (1.5 atm * 101325 Pa/atm = 151987.5 Pa), and the volume to liters (assuming it is given in cm^3 or mL), you can substitute these values into the equation to calculate the mass. Then, you can divide the mass by the volume to get the density in g/L.

Answer 2

The density of freon-11 (CFCl₃) at 120°C and 1.5 atm is 1.477 g/L.

To find this density, we use the formula Density = Mass / Volume.

The mass of freon-11 is determined by its molar mass and the number of moles present in the sample, while the volume is calculated using the ideal gas law.

The molar mass of freon-11 is 137.38 g/mol, and the number of moles is calculated using the ideal gas law equation PV = nRT.

Solving for n:

n = PV / RT

n = (1.5 atm)(V) / (0.08206 L·atm/mol·K)(393.15 K)

n = 0.0535 moles.

With the mass and number of moles known, we can then use the formula Density = Mass / Volume to calculate the density:

Density = (0.0535 mol)(137.38 g/mol) / (V)

This will give the value 1.477 g/L.