A9.000l tank at 27.0°c is filled with 5.29g of sulfur tetrafluoride gas and 15.6g of carbon dioxide 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. round each of your answers to 3 significant digits. sulfur tetraflouride: mole fraction? partial pressure? carbon dioxide: mole fraction? partial pressure? total pressure in tank?

Mole fraction SF₄: 0,121

Mole fraction CO₂: 0,879

Partial pressure SF₄: 0,134 atm

Partial pressure CO₂: 0,968 atm

Total pressure: 1,102 atm

Explanation:

The moles of sulfur tetrafluoride gas and carbon dioxide gas are:

5,29g SF₄×= 0,0489 moles SF₄

15,6 CO₂×= 0,354 moles CO₂

Mole fraction SF₄:

= 0,121

Mole fraction CO₂:

= 0,879

It is possible to obtain partial pressure of both gases with moles of each gas using:

P = nRT/V

Where n are respective moles, R is gas constant (0,082atmL/molK), T is teemperature (27°C=300,15K), V is volume (9,0000L)

Replacing:

Partial pressure SF₄: 0,134atm

Partial pressure CO₂: 0,968atm

Now, the sum of the partial pressures is the total pressure in the tank, that means:

Total pressure: 0,134atm + 0,968atm = 1,102atm

I hope it helps!

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)