Final answer:
The mass of xenon tetrafluoride produced, we need to use the ideal gas law equation to find the number of moles of xenon and fluorine gas. Then, we can use the balanced chemical equation and mole ratio to find the number of moles of xenon tetrafluoride. Finally, by multiplying the number of moles by the molar mass, we can calculate the mass of xenon tetrafluoride.
Step-by-step explanation:
To determine the mass of xenon tetrafluoride produced, we need to use the ideal gas law equation to find the number of moles of xenon and fluorine gas. We can then use the balanced chemical equation for the reaction between xenon and fluorine to find the mole ratio between xenon and xenon tetrafluoride. Finally, we can use the molar mass of xenon tetrafluoride to calculate the mass.
First, we need to convert the temperatures from Celsius to Kelvin by adding 273.15. The initial temperature is 673.15 K. We can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin. Rearranging the equation gives n = PV/RT.
Next, we need to calculate the number of moles of xenon gas. Using the initial pressure of xenon gas (0.500 atm), the volume of the container (20.0 L), the ideal gas constant (0.0821 L·atm/mol·K), and the temperature in Kelvin (673.15 K), we can calculate the number of moles of xenon gas:
n = (0.500 atm) * (20.0 L) / (0.0821 L·atm/mol·K) * (673.15 K) = 0.482 mol
Similarly, we can calculate the number of moles of fluorine gas using the initial pressure of fluorine gas (1.5 atm), the volume of the container (20.0 L), the ideal gas constant (0.0821 L·atm/mol·K), and the temperature in Kelvin (673.15 K):
n = (1.5 atm) * (20.0 L) / (0.0821 L·atm/mol·K) * (673.15 K) = 1.445 mol
Now we use the mole ratio between xenon and xenon tetrafluoride from the balanced chemical equation:
Xe + 2F2 → XeF4
The mole ratio between xenon and xenon tetrafluoride is 1:1, so the number of moles of xenon tetrafluoride produced is also 0.482 mol. Finally, we can calculate the mass of xenon tetrafluoride using its molar mass (207.288 g/mol):
mass = (0.482 mol) * (207.288 g/mol) = 99.94 g