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a tank at is filled with of sulfur tetrafluoride gas and of dinitrogen difluoride gas. you can assume both gases behave as ideal gases under these conditions.

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Mole fraction of N2O is 0.330 and mole fraction of SF4 is 0.669; pressure N2O is 39127.053 Pa ; pressure of SF4 is 792126.36 and total pressure is 118253.413 Pa

What is pressure in chemistry?

If volume and temperature are held constant, ideal gas equation can be rearranged to show that pressure of a sample of gas is directly proportional to number of moles.

Given, volume of tank is 8 L

Weight of dinitrogen difluoride gas is 5.53 g

weight of Sulphur hexafluoride gas is 17.3 g

Amount of N2O= 5.53/ (14 * 2 + 16)

= 0.1256 mol

amount of SF4 = 17.3 /( 32.1 + 19 *4 )

= 0.254 mol

mole fraction of N2O= 0.1256/( 0.1256 + 0.254)

= 0.330

amount of SF4= 0.254/( 0.1256 + 0.254)

= 0.669

PV = n RT

P of N2O = 0.1256* 8.31 ( 273 + 26.9)/0.008

= 39127.053 Pa

mole of SF4 = 0.254* 8.31 ( 273 + 26.9)/0.008

= 79126.36 Pa

Therefore, total pressure  = 39127.053 + 79126.36 = 118253.413 Pa

To know more about pressure in chemistry, refer

https://brainly.com/question/24719118

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Note : The question given on the portal is incomplete. Here is the complete question.

Question : A 8.00 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.

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