At a certain temperature, a mixture of 2 gases, 11.2 g of oxygen and 104.75 of krypton exert a total pressure of 4.25 atm. what is the partial pressure of each gas in mm hg?

Pressure of O₂ = 0.93 atm

Pressure of krypton = 3.32 atm

Explanation:

This problem can be solved 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.

Pₐ = Xₐ * Ptotal

P ₐ  - the partial pressure of component  a  

χ ₐ   - its mole fraction in the mixture

P total  - the total pressure of the mixture

The moles of the two gases are:

moles of O₂ = 11.2/32 = 0.35 moles

moles of krypton = 104.75/83.8 = 1.25 moles

Total moles = 1.25 + 0.35 = 1.6 moles

Xₐ = number of moles of a /total moles in mixture

Pressure of O₂ = 0.35/1.6 *4.25 = 0.93 moles

Pressure of krypton = 1.25/1.6 *4.25 = 3.32 moles

6733.5 g of NaCl

Explanation:

We can assume that the salt solution is a saline solution which contains NaCl in water at 0.90%, whose density is 1.005 g/ml.

So we need to apply the density concept to solve the question.

Density = mass / volume

We convert dL to mL → 67 dL . 100mL / 1 dL = 6700 mL

Density = mass / volume

Volume . Density = mass

6700 mL . 1.005 g = 6733.5 g of NaCl