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A 5.00L tank at −2.4°C is filled with 16.7g of sulfur hexafluoride gas and 8.88g of dinitrogen monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. gas mole fraction sulfur hexafluoride dinitrogen monoxide

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Answer:

X(SF₆) = 0.361

X(N₂O) = 0.639

Explanation:

Step 1: Calculate the moles of each gas

We use the following expression.

n = m / M

where,

  • n: moles
  • m: mass
  • M: molar mass

SF₆: 16.7 g / 146.06 g/mol = 0.114 mol

N₂O: 8.88 g / 44.01 g/mol = 0.202 mol

The total number of moles is 0.114 mol + 0.202 mol = 0.316 mol

Step 2: Calculate the mole fraction of each gas

We use the following expression.

X = moles of gas / total number of moles

X(SF₆) = 0.114 mol / 0.316 mol = 0.361

X(N₂O) = 0.202 mol / 0.316 mol = 0.639

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