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------------------------------------------------ A mixture of gases contains 5.00 grams of Ne, 5.00 grams of O₂, and 5.00 grams of CO₂.

1. What is the mole fraction of each gas?
2. What fraction of the total pressure of the gas mixture is due to each gas?

Assume the gases are in a 25.0 L container at 25°C.

To calculate the mole fraction of each gas, we need to determine the total moles of the mixture. We can do this by dividing each mass by their respective molar masses:

moles of Ne = 5.00 g / 20.18 g/mol = 0.247 mol

moles of O2 = 5.00 g / 32.00 g/mol = 0.156 mol

moles of CO2 = 5.00 g / 44.01 g/mol = 0.113 mol

total moles = 0.247 + 0.156 + 0.113 = 0.516 mol

Now we can calculate the mole fraction of each gas:

mole fraction of Ne = 0.247 mol / 0.516 mol = 0.478

mole fraction of O2 = 0.156 mol / 0.516 mol = 0.302

mole fraction of CO2 = 0.113 mol / 0.516 mol = 0.220

To determine the fraction of the total pressure of the gas mix due to each gas, we need to apply Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each gas:

total pressure = PNe + PO2 + PCO2

The partial pressure of each gas is equal to its mole fraction multiplied by the total pressure of the gas mixture:

PNe = mole fraction of Ne x total pressure = 0.478 x 1.00 atm = 0.478 atm

PO2 = mole fraction of O2 x total pressure = 0.302 x 1.00 atm = 0.302 atm

PCO2 = mole fraction of CO2 x total pressure = 0.220 x 1.00 atm = 0.220 atm

Therefore,To calculate the mole fraction of each gas, we need to determine the total moles of the mixture. We can do this by dividing each mass by their respective molar masses:

moles of Ne = 5.00 g / 20.18 g/mol = 0.247 mol

moles of O2 = 5.00 g / 32.00 g/mol = 0.156 mol

moles of CO2 = 5.00 g / 44.01 g/mol = 0.113 mol

total moles = 0.247 + 0.156 + 0.113 = 0.516 mol

Now we can calculate the mole fraction of each gas:

mole fraction of Ne = 0.247 mol / 0.516 mol = 0.478

mole fraction of O2 = 0.156 mol / 0.516 mol = 0.302

mole fraction of CO2 = 0.113 mol / 0.516 mol = 0.220

To determine the fraction of the total pressure of the gas mix due to each gas, we need to apply Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each gas:

total pressure = PNe + PO2 + PCO2

The partial pressure of each gas is equal to its mole fraction multiplied by the total pressure of the gas mixture:

PNe = mole fraction of Ne x total pressure = 0.478 x 1.00 atm = 0.478 atm

PO2 = mole fraction of O2 x total pressure = 0.302 x 1.00 atm = 0.302 atm

PCO2 = mole fraction of CO2 x total pressure = 0.220 x 1.00 atm = 0.220 atm

ThereforeTo calculate the mole fraction of each gas, we need to determine the total moles of the mixture. We can do this by dividing each mass by their respective molar masses:

moles of Ne = 5.00 g / 20.18 g/mol = 0.247 mol

moles of O2 = 5.00 g / 32.00 g/mol = 0.156 mol

moles of CO2 = 5.00 g / 44.01 g/mol = 0.113 mol

total moles = 0.247 + 0.156 + 0.113 = 0.516 mol

Now we can calculate the mole fraction of each gas:

mole fraction of Ne = 0.247 mol / 0.516 mol = 0.478

mole fraction of O2 = 0.156 mol / 0.516 mol = 0.302

mole fraction of CO2 = 0.113 mol / 0.516 mol = 0.220

To determine the fraction of the total pressure of the gas mix due to each gas, we need to apply Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each gas:

total pressure = PNe + PO2 + PCO2

The partial pressure of each gas is equal to its mole fraction multiplied by the total pressure of the gas mixture:

PNe = mole fraction of Ne x total pressure = 0.478 x 1.00 atm = 0.478 atm

PO2 = mole fraction of O2 x total pressure = 0.302 x 1.00 atm = 0.302 atm

PCO2 = mole fraction of CO2 x total pressure = 0.220 x 1.00 atm = 0.220 atm

Therefore, the fraction of the total pressure of the gas mix due to Ne is 0.478, due to O2 is 0.302, and due to CO2 is 0.220.

Note that we are not given the temperature of the gas mixture, so we cannot calculate the individual partial pressures using the ideal gas law.

Note that we are not given the temperature of the gas mixture, so we cannot calculate the individual partial pressures using the ideal gas law.

Note that we are not given the temperature of the gas mixture, so we cannot calculate the individual partial pressures using the ideal gas law.

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