Question

An ideal gas in a sealed container has an initial volume of 2.60 L. At constant
pressure, it is cooled to 23.00 degrees Celcius, where its final volume is 1.75 L. What
was the initial temperature?


_____

Oho bade Tezz ho xD
​

Answer 1

Explanation:

Answer:-

Given:-

Initial volume of the gas (V₁) = 2.60 L

Final Volume of the gas (V₂) = 1.75 L

Final Temperature (T₂) = 23.00° C = 23 + 273° K = 296° K

[ ∵ °K = °C + 273 ]

We know that,

Charle's law of gases states that at constant pressure, the volume of a gas is directly proportional to its temperature.

That is,

⟹ V ∝ T

⟹ V/T = k (constant)

So,

⟹ V₁/T₁ = V₂/T₂

Let the Initial temperature be T₁.

Hence,

⟹ (2.60)/T₁ = (1.75)/(296)

⟹ (2.60)(296) = T₁ * (1.75)

⟹ (296)(2.60) / 1.75 = T₁

⟹ 439.77° K = T₁

⟹ T₁ = 439.77 - 273°

⟹ T₁ = 166.77° C

∴ The Initial temperature of the gas was 166.77° C.

Answer 2

$\huge\mathbb\fcolorbox{Green}{yellow}{♡ᎪղՏωᎬя᭄}$

Constant pressure is an example of Charles' Law where V1/T1 = V2/T2

(2.65 L)/(T1) = (1.75 L)/(291 K)

T1 = ((2.65 L)(291 K)/1.75 L) = 440 K 

440K - 273 = 168ºC

Learn More:-

Charles's law is an experimental gas law that describes how gases tend to expand when heated. A modern statement of Charles's law is: When the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be in direct proportion.

Since pressure is kept constant, the only variable that is manipulated is temperature. This means that we can use Charles's law in order to compare volume and temperature. Since volume and temperature are on opposite sides of the ideal gas law, they are directly proportional to one another.

❤