Question

A gas is in a sealed balloon is held under isobaric conditions. The initial temperature is 20.°C and the volume is 10.0 L. If the balloon expands to 15.0L, what is the final temperature in °C?

Answer 1

The final temperature in °C = 166.6 °C.

Step-by-step explanation

Given:

Initial temperature, T₁ = 20.0 °C

Initial volume, V₁ = 10.0 L

Final volume, V₂ = 15.0 L

What to find:

The final temperature in °C.

Step-by-step solution:

Since is held under isobaric conditions i.e constant pressure, the final temperature can be determined using the Charle's law equation below.

`\begin{gathered} (V_1)/(T_1)=(V_2)/(T_2) \\ \\ \Rightarrow T_2=(T_1V_2)/(V_1) \end{gathered}`

Plugging T₁ = (20.0 + 273.15) = 293.15 K, V₁ = 10.0 L and V₂ = 15.0 L into the equation, we have

`T_2=\frac{293.15\text{ }K*15.0\text{ }L}{10.0\text{ }L}=439.725K`

The final step is to convert the temperature from Kelvin to °C.

The final temperature = (439.725 - 273.15) = 166.6 °C.