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The problem provided deals with the relationship between temperature and volume at constant pressure. We can solve it using **Charles's Law**, which states that:

\[
\frac{V_1}{T_1} = \frac{V_2}{T_2}
\]

Where:
- \( V_1 \) = initial volume = 1.00 L
- \( T_1 \) = initial temperature = 25°C = 298.15 K (temperature must be in Kelvin)
- \( V_2 \) = final volume (what we're solving for)
- \( T_2 \) = final temperature = 40°C = 313.15 K

Now, let's solve for \( V_2 \):

\[
V_2 = V_1 \times \frac{T_2}{T_1}
\]

Substitute the values:

\[
V_2 = 1.00 \, \text{L} \times \frac{313.15 \, \text{K}}{298.15 \, \text{K}}
\]

I will now calculate the result.The new volume of the balloon, after being heated to 40°C, is approximately **1.05 liters**.

Would you like more details or have any further questions?

Here are 5 related questions to explore this concept further:
1. How would the volume change if the balloon were cooled to 0°C instead of heated?
2. What happens to the pressure in the balloon if the volume were kept constant while heating it?
3. How is Charles's Law related to the Ideal Gas Law?
4. If the balloon was filled with a different gas, would this affect the final volume under the same conditions?
5. What assumptions are made when applying Charles's Law to real gases?

**Tip**: Always remember to convert temperatures to Kelvin when working with gas law equations!

A balloon at 25°C has 1.00 L of air. The balloon is heated to 40°C at constant pressure. What is the new volume?

Solve a Charles's Law problem where a balloon at 25°C with a volume of 1.00 L is heated to 40°C at constant pressure. Learn how to calculate the new volume using the formula V2 = V1 × (T2/T1). Ideal for high school students learning about gas laws.

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