# and 7.55A 10.0 L tank at 3.4 °C is filled with 19.9of dinitrogen difluoride gas. You can assume both gases behave as ideal gasesof boron trifluoridegasunder 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.mole fraction:x10oloboron trifluoride?atmpartial pressure:18Armole fraction:dinitrogen difluoridepartial pressure:atmatmTotal pressure in tank:ExplanationCheck2019 McGraw-Hill Education. All Rights Reserved. Terms of UsePrivacyEscHometnsertEndF4FnLockF12F8F2F3Fi1F6F10F5F7F9&soedey367211XLO

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Calculate the mole faction and partial pressure of each gas and the total pressure in the tank round each of your answer to three significant digits please round only for the final answers not for the math.

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Step 1

The molar mass of boron trifluoride is 67.82 g/mol. The number of moles (n) of boron trifluoride is calculated in equation (1).

The molar mass of dinitrogen difluoride is 66.01 g/mol. The number of moles (n) of dinitrogen difluoride is calculated in equation (2).

Step 2

The mole fraction of boron trifluoride is calculated below.

Step 3

The relation between degree Celsius (○C)and Kelvin (K) is expressed below.

T(K) = 273 + T(○C)

Use the above relation and Convert 3.4 degrees Celsius.

T (K) = 273 + 3.4○C

T(K) = 276.4 K

The partial ...

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