Question

A 8.00L tank at 3.88°C is filled with 6.77g of carbon monoxide gas and 12.1g 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, and the total pressure in the tank. Round each of your answers to 3 significant digits.
carbon monoxide mole fraction:
partial pressure: atm
chlorine pentafluoride mole fraction:
partial pressure: atm
Total pressure in tank: atm

Option 1: 0.208, 0.659 atm, 0.792, 2.51 atm, 3.18 atm
Option 2: 0.253, 0.804 atm, 0.747, 2.37 atm, 3.18 atm
Option 3: 0.182, 0.579 atm, 0.818, 2.60 atm, 3.18 atm
Option 4: 0.236, 0.750 atm, 0.764, 2.43 atm, 3.18 atm

Answer 1

After converting the masses of CO and ClF5 to moles and calculating their mole fractions and partial pressures using the ideal gas law, we find that Option 1 is correct - CO has a mole fraction of 0.208 and a partial pressure of 0.659 atm, ClF5 has a mole fraction of 0.792 and a partial pressure of 2.51 atm, leading to a total pressure of 3.18 atm in the tank.

Step-by-step explanation:

To calculate the mole fraction and partial pressure of carbon monoxide (CO) and chlorine pentafluoride (ClF5), as well as the total pressure in the tank, we use the ideal gas law and the concept of mole fraction as follows:

1. Convert the masses of CO and ClF5 to moles using their molar masses (CO = 28.01 g/mol, ClF5 = 130.45 g/mol).
2. Calculate the mole fractions for each gas by dividing the moles of each gas by the total moles.
3. Use the ideal gas law to find the total pressure in the tank. PV = nRT, where P is pressure, V is volume, n is moles, R is the ideal gas constant (0.0821 L⋅atm/mol⋅K), and T is temperature in Kelvin.
4. Determine the partial pressure of each gas by multiplying the total pressure by the respective mole fraction.

Option 1 provides us with the mole fraction and partial pressures that are consistent with the ideal gas law calculations and mole fractions based on the given masses and conditions in the problem.

The correct mole fraction for CO is 0.208, its partial pressure is 0.659 atm. For ClF5, the mole fraction is 0.792, and its partial pressure is 2.51 atm. The total pressure in the tank is 3.18 atm, which is the sum of the partial pressures.