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erastova [34]
3 years ago
13

A balloon contains 146.0mL of gas confined at a pressure of 1.30atm and a temperature of 5.00ºC. If the pressure changes to 2.60

atm and the temperature decreases to 2.00ºC, what will be the volume of gas in the balloon?
Chemistry
1 answer:
Talja [164]3 years ago
4 0

Answer:

V₂ = 72.2 mL

Explanation:

Given data:

Initial volume = 146.0 mL

Initial pressure = 1.30 atm

Initial temperature = 5.00 °C (5.00 +273 = 278 K)

Final temperature = 2.00  °C ( 2.00+273 = 275 K)

Final volume = ?

Final pressure = 2.60 atm

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

P₁V₁/T₁ = P₂V₂/T₂  

V₂ = P₁V₁T₂  /T₁P₂

V₂ = 1.30 atm × 146.0 mL × 275 K / 278K × 2.60 atm

V₂ = 52195  atm .mL. K / 722.8 K.atm

V₂ = 72.2 mL

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8.03 solutions report is described below.

Explanation:

8.03 Solutions Lab Report

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A solution of methanol and water has a mole fraction of water of 0.312 and a total vapor pressure of 211 torr at 39.9 ºC. The va
r-ruslan [8.4K]

Answer:

The solution is not ideal.

The relative strengths of the solute-solvent interactions are greater  compared to the solute-solute and solvent-solvent interactions

Explanation:

The total vapor pressure is the sum of the partial pressures of  water and methanol, and they are calculated by the Raoult´s law equation:

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The final concentration is 1.5 M
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