Answer: -
1.34 L
Explanation: -
Initial Pressure P 1 = 39.1 bar
Initial Temperature T 1 = 643 K
Let the initial volume be V 1.
Final pressure P 2 = 87.0 bar
Final temperature T 2 = 525 K.
Final volume V 2 = 0.492 L
Using the equation
[tex] \frac{P1 V 1}{T1} = \frac{P 2 V 2}{T2} [/tex]
[tex] V 1 = \frac{P2 V2 T1}{P 1 T2} [/tex]
Plugging in the values
We have
V 1 = 87 bar x 0.492 L x 643 K / (39.1 bar x 525 K)
= 1.34 L
Thus, a gas is contained in a thick-walled balloon. When the pressure changes from 39.1 bar to 87.0 bar the volume changes from 1.34 L to 0.492L and the temperature changes from 643K to 525K
P₁ = 39.1 bar
V₁ = ?
T₁ = 643 K
P₂ = 87.0 bar
V₂ = 0.492 L
T₂ = 515 K
P₂ = ?
P₁V₁/T₁ = P₂V₂/T₂
V₁ = P₂V₂T₁/P₁T₂ = (87.0)(0.492)(643) / (39.1)(515) = 1.37 L
