Uranium hexafluoride is a solid at room temperature, but it boils at 56°C. Determine the density of uranium hexafluoride at 76°C at 747 torr.
To determine the density of uranium hexafluoride at 76°C and 747 torr, we need to use the ideal gas law.
The ideal gas law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the temperature from Celsius to Kelvin. The conversion from Celsius to Kelvin is given by the formula: K = °C + 273.15.
Let's convert the temperature:
T = 76°C + 273.15 = 349.15 K
Now let's convert the pressure from torr to atmospheres (atm). Remember that 1 atm = 760 torr.
P = 747 torr / 760 torr/atm = 0.9816 atm
Next, we need to determine the molar mass of uranium hexafluoride (UF6) which is composed of one uranium atom (U) and six fluorine atoms (F). The molar mass of uranium is 238.03 g/mol, and the molar mass of fluorine is 18.998 g/mol.
Molar mass of UF6 = (238.03 g/mol) + 6 * (18.998 g/mol) = 352.03 g/mol
Now, let's rearrange the ideal gas law equation to solve for density, which is mass/volume:
PV = nRT
n = PV/RT
n = (0.9816 atm) * V / [(0.0821 L·atm/mol·K) * 349.15K]
n = (0.9816 atm) * V / 28.732 L·atm/mol
n = 0.03408 V / L·mol
Next, we can substitute the molar mass to calculate the mass of the uranium hexafluoride:
m = n * Molar mass
m = (0.03408 V / L·mol) * (352.03 g/mol)
m = 11.995 g * V / L
Finally, we can rearrange the density equation to solve for density:
density = mass / volume
density = (11.995 g * V / L) / V
density = 11.995 g / L
Therefore, at 76°C and 747 torr, the density of uranium hexafluoride is approximately 11.995 g/L.
To determine the density of uranium hexafluoride (UF6) at a specific temperature and pressure, we need to use the ideal gas law equation. The ideal gas law is expressed as:
PV = nRT
Where:
P = pressure of the gas
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin
First, we need to convert the given temperature from Celsius to Kelvin. The conversion formula is:
T(K) = T(°C) + 273.15
So, the temperature T in Kelvin is:
T = 76°C + 273.15 = 349.15 K
Next, we need to convert the given pressure from torr to atmospheres. 1 atm is equal to 760 torr. The conversion formula is:
P(atm) = P(torr) / 760
So, the pressure P in atmospheres is:
P = 747 torr / 760 = 0.9816 atm
Now, we can rearrange the ideal gas law equation to solve for the number of moles (n) of uranium hexafluoride:
n = PV / RT
To calculate n, we will need to know the volume (V) of uranium hexafluoride. However, this information is not provided in the question. Therefore, we cannot determine the number of moles and, consequently, the density of uranium hexafluoride at the given conditions.
In summary, without the volume information, we cannot calculate the density of uranium hexafluoride at 76°C and 747 torr.
P*molar mass = density*RT
Solve for density.