A8.00 l tank at 26.9 c is filled with 5.53 g of dinitrogen difluoride gas and 17.3 g of sulfur hexafluoride 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

mole fraction of N_2 O = 0.330

mole of fraction SF_4 = 0.669

PRESSURE OF N_2 O = 39127.053 Pa

pressure of SF_4 = 792126.36

Total pressure   = 118253.413 Pa

Explanation:

Given data:

volume of tank 8 L

Weight of dinitrogen difluoride gas 5.53 g

weight of sulphur hexafluoride gas 17.3 g

Amount of

amount of

mole fraction of

mole of fraction

PV = nRT

P of N_2 O

mole of SF_4

Total pressure  = 39127.053 + 79126.36 = 118253.413 Pa

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