A mixture of He, N,, and Ar has a pressure of 13.5 atm at 28.0 °C. If the partial pressure of He is 1097 torr and that of Ar is 3019 mm Hg, what is the partial pressure of N, ? PN, atm

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A mixture of He, N₂, and Ar has a pressure of 13.5 atm at 28.0 °C. If the partial pressure of He is 1097 torr and that of Ar is 3019 mm Hg, what is the partial pressure of N₂?

\[ P_{N_2} = \text{\_\_\_\_\_\_\_\_\_\_\_\_\_} \, \text{atm} \]
Transcribed Image Text:A mixture of He, N₂, and Ar has a pressure of 13.5 atm at 28.0 °C. If the partial pressure of He is 1097 torr and that of Ar is 3019 mm Hg, what is the partial pressure of N₂? \[ P_{N_2} = \text{\_\_\_\_\_\_\_\_\_\_\_\_\_} \, \text{atm} \]
Expert Solution
Step 1

Consider the given information is as follows;

Total pressure ptotal = 13.5 atm    

Partial pressure of He pHe1097 torr = 1097760=1.44 atm

Partial pressure of Ar pAr3019 mmHg = 3019760=3.97 atm   

Partial pressure of N2 pN2 = ?

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