A mixture of He, Ar and Xe has a total pressure of 2.00 atm. The partial pressure of He is .450 atm, Ar partial pressure is 0.400. What is the partial pressure of Xe?

P(Xe) = 1.15 atm

Explanation:

Given data:

Total pressure = 2.00 atm

Partial pressure of He = 0.450 atm

Partial pressure of Ar  = 0.400 atm

Partial pressure of Xe = ?

Solution:

According to Dalton law of partial pressure,

The total pressure inside container is equal to the sum of partial pressures of individual gases present in container.

Mathematical expression:

P(total) = P₁ + P₂ + P₃+ +Pₙ

Now we will solve this  problem by using this law.

P(total) = P(He) + P(Ar) + P(Xe)

2.00 atm = 0.450 atm + 0.400 atm + P(Xe)

2.00 atm = 0.850 atm + P(Xe)

P(Xe) = 2.00 atm - 0.850 atm

P(Xe) = 1.15 atm

h let me think

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: