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A gas has a volume of 4.54 L at 1.65 atm and 75.0°C. At what pressure would the volume

of the gas be increased to 5.33 L if the temperature is increased to 103°C?

Respuesta :

ysabayomi

Answer:

The correct answer is 1.52 atm

Explanation:

The formula to be used here is that of the combined gas law

P₁V₁/T₁ = P₂V₂/T₂

where

P₁ is the initial pressure (1.65 atm)

V₁ is the initial volume (4.54 L)

T₁ is the initial temperature (must be converted to kelvin) 75°C + 273 = 348K

P₂ is the final pressure (unknown)

V₂ is the final volume (5.33 L)

T₂ is the final temperature (must be converted to kelvin) 103°C + 273 = 376K

1.65 × 4.54/348 = P₂ × 5.33/376

P₂ = 1.65 × 4.54 × 376 ÷ 5.33 × 348

P₂ = 2816.62 ÷ 1854.84

P₂ = 1.52 atm

samueladesida43

The new pressure of a gas that has a volume of 4.54 L at 1.65 atm and 75.0°C is 1.52atm.

How to calculate pressure?

The new pressure of a gas can be calculated by using the following expression:

P1V1/T1 = P2V2/T2

Where;

  • P1 and P2 = initial and final pressure respectively
  • V1 and V2 = initial and final volume respectively
  • T1 and T2 = initial and final temperature respectively

  1. T1 = 75°C + 273 = 348K
  2. T2 = 103°C + 273 = 376K

1.65 × 4.54/348 = P2 × 5.33/376

0.0215 = 0.014P2

P2 = 0.0215 ÷ 0.014

P2 = 1.52atm

Therefore, the new pressure of a gas that has a volume of 4.54 L at 1.65 atm and 75.0°C is 1.52atm.

Learn more about pressure at: https://brainly.com/question/4631715

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