# A 7.00 L tank at 12.5 °C is filled with 12.5 g of dinitrogen difluoride gas and 19.4 g of boron trifluoride gas. You can assume both gases behave as ideal gasesunder these conditions.Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits.mole fractiongasS?dinitrogen difluorideboron trifluorideArExplanationCheck© 2019 McGraw-Hill Education. All Rights Reserved.Terms of UsePrivacye11:13 PMOType here to search99+Pxp12/3/2019hpBaf10IIf9insprt scf8fi1f12f6f5pg upendf4homedeleteesc&@2\$#numOCO7backspace6135lockIILO26

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Step 1

To calculate the mole fraction of each gas, first it is required to calculate the number of moles of each gas present, which can be done as,

Step 2

The mass of N2F2 is given as 12.5 g and that of BF3 is 19.4 g. T...

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