Asample of argon fills a volume of 5 m3 at 425 k with a pressure of 3.9 atm. the argon is cooled to 240 k and shrinks to a volume of 3.1 m3. after cooling it is added to a tank of helium with a pressure of 1.87 atm. what is the total pressure of the gas mixture? a. 3.55 atm b. 2.89 atm c. 13.0 atm d. 5.42 atm

D. 5.42 atm.

Explanation:

The total pressure of the gas mixture = P of He + P of Ar after cooling.

P of He = 1.87 atm.

We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R  is the general gas constant,

T is the temperature of the gas in K.

(P₁V₁T₂) = (P₂V₂T₁)

P₁ = 3.9 atm, V₁ = 5.0 m³, T₁ = 425.0 K,

P₂ = ??? atm, V₂ = 3.1 m³, T₂ = 240.0 K,

(P₁V₁T₂) = (P₂V₂T₁)

∴ P₂ = (P₁V₁T₂)/(V₂T₁) = (3.9 atm)(5.0 m³)(240 K)/(3.1 m³)(425.0 K) = 3.552 atm.

∴ The total pressure of the gas mixture = P of He + P of Ar after cooling.

P of He = 1.87 atm & P of Ar after cooling = 3.552 atm.

∴ The total pressure of the gas mixture = 1.87 atm + 3.552 atm = 5.422 atm ≅ 5.42 atm.

So, the right choice is: D. 5.42 atm.

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a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.