Question

9g of helium and 0.4g of oxygen...........find the number of atom.....
need stepssss plzzz exam is going on

Answer 1

Explanation:

You can solve this problem by using Dalton's Law of Partial Pressures, which states that the partial pressure of a component of a gaseous mixture depends on the mole ratio of said component and the total pressure of the gaseous mixture.

∣∣ ∣∣¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯aaPi=χi×Ptotalaa∣∣−−−−−−−−−−−−−−−−−−, where

Pi - the partial pressure of component i

χi - its mole fraction in the mixture

Ptotal - the total pressure of the mixture

Since you already know the total pressure of the mixture, focus on finding how many moles of each gas you get in the mixture.

To do that, use the molar masses of the two gases. You will havewill have

54.5g⋅1 mole O232.0g=1.703 moles O2

68.9g⋅1 mol CO244.01g=1.566 moles CO2

The total number of moles present in the mixture will be

ntotal=nO2+nCO2

ntotal=1.703 moles+1.566 moles=3.269 moles

Now, to get the mole fraction of a gas i that's part of a mixture, simply divide the number of moles of that gas by the total number of moles present in the mixture

Answer 2

Answer:

answer is

Explanation:

i dnt know sorry