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yuradex [85]
3 years ago
5

A plastic bottle is closed outdoors on a cold day when the temperature is −15.0°C and is later brought inside where the temperat

ure is 21.5°C. What is the pressure of the air in the bottle after it reaches room temperature, assuming the air in the bottle was at a pressure of 1.00 atm upon reaching thermal equilibrium with the outdoor temperature?
Chemistry
1 answer:
Lana71 [14]3 years ago
3 0

Answer:

Pressure = 1.14 atm

Explanation:

Hello,

This question requires us to calculate the final pressure of the bottle after thermal equilibrium.

This is a direct application of pressure law which states that in a fixed mass of gas, the pressure of a given gas is directly proportional to its temperature, provided that volume remains constant.

Mathematically, what this implies is

P = kT k = P / T

P1 / T1 = P2 / T2 = P3 / T3 =........= Pn / Tn

P1 / T1 = P2 / T2

P1 = 1.0atm

T1 = -15°C = (-15 + 273.15)K = 258.15K

P2 = ?

T2 = 21.5°C = (21.5 + 273.15)K = 294.65K

P1 / T1 = P2 / T2

P2 = (P1 × T2) / T1

P2 = (1.0 × 294.65) / 258.15

P2 = 1.14atm

The pressure of the gas after attaining equilibrium is 1.14atm

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On a summer day early in the moming, a balloon is filled with helium when the temperature
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Based on the data provided;

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  • pressure at peak temperature is 259.3 kPa
  • internal pressure is above 256 kPa, therefore, the balloon will burst.
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<h3>What is the ideal has equation?</h3>

The ideal gas equation relatesthe pressure, volume, moles and temperature of a gas.

The moles of helium gas is calculated using the Ideal gas equation:

  • PV = nRT

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The pressure should be reduced to a value less than 256 kPa by reducing the temperature.

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