A 6.00L tank at 10.7°C is filled with 5.94g of sulfur tetrafluoride gas and 9.47g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions.Calculate the mole fraction and partial pressure of each gas in the tank. Round each of your answers to 3 significant digits
Question
A 6.00L tank at 10.7°C is filled with 5.94g of sulfur tetrafluoride gas and 9.47g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions.Calculate the mole fraction and partial pressure of each gas in the tank. Round each of your answers to 3 significant digits
Solution
To solve this problem, we first need to calculate the number of moles of each gas, then the total pressure, and finally the mole fraction and partial pressure of each gas.
Step 1: Calculate the number of moles of each gas
The molar mass of sulfur tetrafluoride (SF4) is approximately 108 g/mol and the molar mass of sulfur hexafluoride (SF6) is approximately 146 g/mol.
Number of moles of SF4 = mass / molar mass = 5.94 g / 108 g/mol = 0.055 mol Number of moles of SF6 = mass / molar mass = 9.47 g / 146 g/mol = 0.065 mol
Step 2: Calculate the total pressure
We can use the ideal gas law (PV = nRT) to calculate the total pressure. We know the volume (V = 6.00 L), the temperature (T = 10.7°C = 283.85 K), and the gas constant (R = 0.0821 L·atm/(mol·K)). The total number of moles (n) is the sum of the moles of SF4 and SF6.
n = 0.055 mol + 0.065 mol = 0.12 mol
P = nRT / V = (0.12 mol * 0.0821 L·atm/(mol·K) * 283.85 K) / 6.00 L = 0.571 atm
Step 3: Calculate the mole fraction and partial pressure of each gas
The mole fraction of a gas is the number of moles of that gas divided by the total number of moles. The partial pressure of a gas is the mole fraction of that gas times the total pressure.
Mole fraction of SF4 = 0.055 mol / 0.12 mol = 0.458 Mole fraction of SF6 = 0.065 mol / 0.12 mol = 0.542
Partial pressure of SF4 = 0.458 * 0.571 atm = 0.262 atm Partial pressure of SF6 = 0.542 * 0.571 atm = 0.309 atm
So, the mole fraction of SF4 is 0.458 and its partial pressure is 0.262 atm. The mole fraction of SF6 is 0.542 and its partial pressure is 0.309 atm.
Similar Questions
A 10.0L tank at 0.89°C is filled with 13.2g of chlorine pentafluoride gas and 16.0g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions.Calculate the mole fraction and partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits.chlorine pentafluoride mole fraction: partial pressure: atmsulfur tetrafluoride mole fraction: partial pressure: atm
A 8.00L tank at 0.84°C is filled with 8.83g of dinitrogen monoxide gas and 17.0g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions.Calculate the mole fraction and partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits.dinitrogen monoxide mole fraction: partial pressure: atmchlorine pentafluoride mole fraction: partial pressure: atm
A 7.00L tank at 24.9°C is filled with 5.16g of chlorine pentafluoride gas and 4.17g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions.Calculate the total pressure in the tank. Round your answer to the correct number of significant digits.
A reaction at 25.0°C evolves 497.mmol of sulfur tetrafluoride gas.Calculate the volume of sulfur tetrafluoride gas that is collected. You can assume the pressure in the room is exactly 1atm. Be sure your answer has the correct number of significant digits
A reaction between liquid reactants takes place at −3.0°C in a sealed, evacuated vessel with a measured volume of 5.0L. Measurements show that the reaction produced 17.g of sulfur tetrafluoride gas.Calculate the pressure of sulfur tetrafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.