Question
Asked Nov 15, 2019
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A 7.00L tank at 22.6°C is filled with 4.26g of dinitrogen difluoride gas and 2.49g of carbon dioxide 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
dinitrogen difluoride
 
carbon dioxide
 

 

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Expert Answer

Step 1

The mass of nitrogen difluoride is 4.26 g and that of carbon dioxide is 2.49 g. To calculate the mole fraction of each gas, it is required to calculate the number of moles of each gas,

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Mass Number of moles Molecular Mass Molecular mass of N2F2 = 14 x 2 19 x 2 = 66 g/mol Molecular mass of CO2 1216 x 2 44 g/mol

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Step 2

Calculating the number of moles of the gases,

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Mass Number of moles Molecular Mass 4.26 Number of moles of N2F2 66 Number of moles of N2F2 0.0645 2.49 Number of moles of CO2 44 Number of moles of CO2 = 0.0565

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Step 3

Now calculating the mole fraction o...

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Moles of nitrogen difluoride Mole fraction of N2F2 Moles of nitrogen difluoride + moles of carbon dioxide 0.0645 Mole fraction of N2F2 0.0565 0.0645 Mole fraction of N2F2 0.533

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