SAMPLE PROBLEM : CHARLES' LAW If I have 45 liters of helium in a balloon at \( 25 \mathrm{~K} \) and increase the temperature of the balloon to \( 55 \mathrm{~K} \), what will the new volume of the balloon be? If I have 45 liters \( \left(V_{1}\right) \) of helium in a balloon at
Added by Juan Diego R.
Close
Step 1
The initial volume (V1) is 45 liters and the initial temperature (T1) is 25 K. The final temperature (T2) is 55 K. Show more…
Show all steps
Your feedback will help us improve your experience
Narayan Hari and 99 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
A balloon is inflated with helium to a volume of $4.5 \mathrm{~L}$ at $23{ }^{\circ} \mathrm{C}$. If you take the balloon outside on a cold day $\left(-10 .{ }^{\circ} \mathrm{C}\right)$, what will be the new volume of the balloon?
A sample of gas occupies an initial volume of 4.9 L at an initial temperature of 315 K. The gas is heated to 350 K while the pressure and the amount of gas remain constant. Which gas law(s) could you apply to determine the new volume of the gas?
Ronald P.
The air inside a balloon is heated to $45^{\circ} \mathrm{C}$ and then cools to $25^{\circ} \mathrm{C} .$ By what percentage does the volume of the balloon change during cooling?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Watch the video solution with this free unlock.
EMAIL
PASSWORD