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5. A scuba driver has a 10 L tank that is filled with Nitrox or otherwise known as "enriched air. Therefore, it contains 5.00 g of oxygen gas (O2) and 8.31 g of nitrogen gas (N2). The pressure of the tank is 179.6 atm. What is the partial pressure of both oxygen and nitrogen?

User Yunus ER
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1 Answer

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Answer : The partial pressure of both oxygen and nitrogen is, 61.8 atm and 117.8 atm respectively.

Explanation :

First we have to calculate the moles of
O_2 and
N_2


\text{Moles of }O_2=\frac{\text{Given mass }O_2}{\text{Molar mass }O_2}=(5.00g)/(32g/mol)=0.156mol

and,


\text{Moles of }N_2=\frac{\text{Given mass }N_2}{\text{Molar mass }N_2}=(8.31g)/(28g/mol)=0.297mol

Now we have to calculate the mole fraction of
O_2 and
N_2


\text{Mole fraction of }O_2=\frac{\text{Moles of }O_2}{\text{Moles of }O_2+\text{Moles of }N_2}


\text{Mole fraction of }O_2=(0.156)/(0.156+0.297)=0.344

and,


\text{Mole fraction of }N_2=\frac{\text{Moles of }N_2}{\text{Moles of }O_2+\text{Moles of }N_2}


\text{Mole fraction of }O_2=(0.297)/(0.156+0.297)=0.656

Now we have to calculate the partial pressure of both oxygen and nitrogen.

According to the Raoult's law,


p_i=X_i* p_T

where,


p_i = partial pressure of gas


p_T = total pressure of gas = 179.6 atm


X_i = mole fraction of gas


p_(O_2)=X_(O_2)* p_T


p_(O_2)=0.344* 179.6atm=61.8atm

and,


p_(N_2)=X_(N_2)* p_T


p_(N_2)=0.656* 179.6atm=117.8atm

Thus, the partial pressure of both oxygen and nitrogen is, 61.8 atm and 117.8 atm respectively.

User Divided
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