Answer :

Final answer:

To find the total pressure of a gas mixture, you need to calculate the moles of each gas using their molar masses and then use the ideal gas law to solve for the pressure.

Explanation:

A gas mixture contains 1.31 g N2 and 1.57 g O2 in a 1.17 L container at 13 ∘C. To solve this problem, we need to calculate the moles of N2 and O2 using their molar masses. Then, we can use the ideal gas law to find the total pressure of the gas mixture.

  1. Calculate the moles of N2 using its molar mass: moles of N2 = mass of N2 / molar mass of N2.
  2. Calculate the moles of O2 using its molar mass: moles of O2 = mass of O2 / molar mass of O2.
  3. Use the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the moles, R is the ideal gas constant, and T is the temperature (in Kelvin) to find the total pressure of the gas mixture. Rearrange the equation to solve for P: P = (nN2 + nO2)RT / V.

Substitute the known values into the equation and calculate the total pressure.

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Completed Question:
A gas mixture contains 1.25 g N2 and 0.85 g O2 in a 1.55 L container at 18 C.

a. Calculate the mole fraction of each component of the mixture.

b. Calculate the partial pressure of each component of the mixture.

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