Question

If .654 g of oxygen dissolves in 1.5 L of water at 1.65 atm, at what pressure would you be able to dissolve 1.35 g in the same amount of water?

Answer 1

Answer: 3.41

Step-by-step explanation:

Answer 2

`P_2=3.41atm`

Step-by-step explanation:

Hello,

In this case, we first compute the moles of oxygen in 0.654 g and 1.35 g by using its molar mass (32 g/mol):

`n_1=0.654g*(1mol)/(32g) =0.0204mol\\n_2=1.35g*(1mol)/(32g) =0.0422mol`

Then, by using the ideal gas equation at the both states, given the same both temperature and volume:

`V_1=V_2\\\\(n_1RT)/(P_1)=(n_2RT)/(P_2)`

`(n_1)/(P_1)=(n_2)/(P_2)`

We compute the volume at the second moles:

`P_2=(P_1n_2)/(n_1)=(1.65atm*0.0422mol)/(0.0204mol)\\ \\P_2=3.41atm`

Best regards.