Suppose We Have 24.4l Pure Sample Containing 1.0mole Of Oxygen Gas At Pressure Of 0.50atm And Temprerature Of 10\Xb0c. If All Of The Oxygen Gas Were C

Suppose we have 24.4L pure sample containing 1.0mole of Oxygen gas at pressure of 0.50atm and temprerature of 10°C. if all of the oxygen gas were converted into ozome gas, what will be the volume of the ozome produce, considuring that the temprerature and pressure remains the same

 

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Problem:

Suppose we have 24.4L pure sample containing 1.0mole of Oxygen gas at pressure of 0.50atm and temprerature of 10°C. if all of the oxygen gas were converted into ozome gas, what will be the volume of the ozome produce, considuring that the temprerature and pressure remains the same

Note: 1 mole of Oxygen (O2) converted to Ozone (O3) (unknown mole)

                         3O2 → 2O3

        3 moles of O2 will produce 2 moles of O3 (we can used this as a conversion factor:

To find the moles of O3 (ozone):

                 1 mole O2 × 2 moles O3 / 3 moles O2 = 0.67 moles of O3

                           1 mole of O2 = .67 moles (O3)

Given Data:

V1 = 24.4 L                          V2 = ? unknown                    

n1 = 1 mole                           n2 = .67 moles

Solution:

This problem can be solved using Avogadros Law which state that volume is directly proportional to the amount of gas when pressure and temperature are constant.

Formula ;  V1/n1 = V2/n2

V2 = V1n2 / n1

     = 24.4 L × .67 mol / 1 mol   (cancel the unit mol)

V2  = 16.348 L

Answer: Ozone gas will occupy a volume of 16.348 L

Hope this helps....