Question

On a ship sailing in the Pacific ocean, where the temperature is ${23.4}^{\circ }\text{C}$, a balloon is filled with $2\text{L}$ of air. What will be the volume of the balloon when the ship reaches the Indian ocean, where the temperature is ${26.1}^{\circ }\text{C}$?

• A. $2.018\text{L}$
• B. $4.036\text{L}$
• C. $8.72\text{L}$
• D. $9.5\text{L}$

Answer 1

The correct option is A $2.018\text{L}$

Given information:
Initial volume of the balloon $V_1=2$ L
Initial temperature of the balloon $T_1=(23.4+273)=296.4K$
Final temperature of the balloon $T_2=(26.1+273)=299.1K$
Final volume of the balloon $V_2=?$
From Charle's law, $\frac{V_1}{T_1}=\frac{V_2}{T_2}$ at constant pressure.

$\Rightarrow V_2=V_1{T}_2/T_1=\frac{2\times 299.1}{296.4}=2.018\text{L}$