Question

An ideal gas in a sealed container has an initial volume of 2.65 L.

2.65 L. At constant pressure, it is cooled to 15.00 ∘C,

15.00 ∘C, where its final volume is 1.75 L.

1.75 L. What was the initial temperature?

Answer 1

Solution

Since P1 = P2 = Constant we apply Charles' Law

V1 = 2.65L

V2 = 1.75L

T1 = ?

T2 = 15.00^oC + 273K = 288K

$\dfrac{V1}{T1} =\dfrac{V2}{T2}$

Making T1 the subject of the formula gives;

$T1 = \dfrac{T2V1}{V2}$

Substituting gives;

$T1=\dfrac{288K x 2.65L}{1.75L} = 436.144K$

Changing it to ^oC by -273K

T1 (initial temperature)= 163.11^oC