A Chemical Calculation Challenge

Chemical Calculation Exercise

A 7.00L tank at 7.1°C is filled with 15.6g of sulfur tetrafluoride gas and 2.40g of dinitrogen monoxide 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.

Calculation Process

To begin with, we can calculate the number of moles for each gas based on the given masses and molar masses of each compound.

  • For sulfur tetrafluoride (SF4):
    Molar mass of SF4 = 32.06 (S) + 4(19.00) = 108.06 g/mol
    Number of moles of SF4 = 15.6g / 108.06 g/mol = 0.144 moles
  • For dinitrogen monoxide (N2O):
    Molar mass of N2O = 2(14.01) + 16.00 = 44.03 g/mol
    Number of moles of N2O = 2.40g / 44.03 g/mol = 0.054 moles

Mole Fraction Calculation

The mole fraction of each gas can be calculated by dividing the number of moles of each gas by the total moles of gas in the tank.

  • Mole fraction of SF4: 0.144 moles / (0.144 moles + 0.054 moles) = 0.727
  • Mole fraction of N2O: 0.054 moles / (0.144 moles + 0.054 moles) = 0.273

Partial Pressure Calculation

The partial pressure of each gas can be calculated using the ideal gas law, where: Partial Pressure = Moles of Gas * Gas Constant * Temperature / Volume

Partial pressure of SF4: 0.144 moles * 0.0821 L.atm/mol.K * (7.1°C + 273.15)K / 7.00L = 0.212 atm
Partial pressure of N2O: 0.054 moles * 0.0821 L.atm/mol.K * (7.1°C + 273.15)K / 7.00L = 0.081 atm

Total Pressure Calculation

The total pressure in the tank is the sum of the partial pressures of each gas: Total Pressure = Partial Pressure of SF4 + Partial Pressure of N2O Total Pressure = 0.212 atm + 0.081 atm = 0.293 atm

Apa hasil perhitungan total tekanan dalam tangki? Total tekanan dalam tangki adalah 0.293 atm setelah dihitung berdasarkan penjumlahan dari tekanan parsial masing-masing gas.
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