Question

An "empty" container is not really empty if it contains air. How may moles of nitrogen are in an "empty" two-liter cola bottle at atmospheric pressure and room temperature (25∘C)? Assume ideal behavior.What is the partial pressure of oxygen in air at atmospheric pressure (1 atm)? Assume ideal behavior

Answer 1

1. 0.0637 moles of nitrogen.

2. The partial pressure of oxygen is 0.21 atm.

Step-by-step explanation:

1. If we assume ideal behaviour, we can use the Law of ideal gases to find the moles of nitrogen, considering that air composition is mainly nitrogen (78%), oxygen (21%) and argon (1%):

`V_(N_2)=V_(T)* 0.78=2L * 0.78 =1.56 L\\PV=nRT\\n_(N_2)=(PV)/(RT)=(1 atm* 1.56 L)/(0.0821(atmL)/(molK)* 298 K)\\n_(N_2)= 0.0637 mol`

2. Now, in order to find he partial pressure of oxygen we need to find the total moles of air, and then the moles of oxygen. Then, we use these results to determine the molar fraction of oxygen, to multiply it with total pressure and get the partial pressure of oxygen as follows:

`n_(total)=(1 atm * 2L)/(0.0821 (atmL)/(molK)298K)=0.0817 mol`

`V_(O_2)=2L * 0.21 = 0.42 L\\n_(O_2)=\frac {1atm * 0.42 L}{0.0821 (atm L)/(mol K)298 K}=0.0172 mol\\X_(O_2)=(n_(O_2))/(n_(total))=(0.0172 mol)/(0.0817 mol)= 0.21`

`P_(O_2)=X_(O_2) * P = 1 atm * 0.21 = 0.21 atm`

As you see, the molar fraction and volume fraction are the same because of the assumption of ideal behaviour.