An arctic weather balloon is filled with 37.5 L of helium gas inside a prep shed. The temperature inside the shed is 6. °C. The balloon is then taken outside, where the temperature is -31. °C. Calculate the new volume of the balloon.

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### Problem: Calculating the New Volume of a Helium Balloon

An arctic weather balloon is initially filled with 37.5 L of helium gas inside a preparation shed. The initial temperature inside the shed is 6°C. The balloon is then taken outside, where the temperature drops to -31°C. Determine the new volume of the balloon.

Assumption: 
- The pressure on the balloon remains constant at exactly 1 atm.

Approach:
- Use Charles's Law which states that \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \), where V is volume and T is temperature in Kelvin.

Instructions:
- Convert the given temperatures from Celsius to Kelvin.
- Apply Charles's Law to solve for the new volume \( V_2 \).
- Present your answer rounded to 3 significant digits.

### Conversion of Temperatures:
- Initial Temperature \( T_1 \): \( 6°C = 279 \, \text{K} \)
- Final Temperature \( T_2 \): \( -31°C = 242 \, \text{K} \)

### Calculation:
Given:
\( V_1 = 37.5 \, \text{L} \), \( T_1 = 279 \, \text{K} \), \( T_2 = 242 \, \text{K} \)

Using Charles's Law:
\[ \frac{37.5}{279} = \frac{V_2}{242} \]

Solve for \( V_2 \):
\[ V_2 = \frac{37.5 \times 242}{279} \]

### New Volume \( V_2 \):
Calculate the expression to find the approximate volume, rounding to 3 significant digits.
Transcribed Image Text:### Problem: Calculating the New Volume of a Helium Balloon An arctic weather balloon is initially filled with 37.5 L of helium gas inside a preparation shed. The initial temperature inside the shed is 6°C. The balloon is then taken outside, where the temperature drops to -31°C. Determine the new volume of the balloon. Assumption: - The pressure on the balloon remains constant at exactly 1 atm. Approach: - Use Charles's Law which states that \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \), where V is volume and T is temperature in Kelvin. Instructions: - Convert the given temperatures from Celsius to Kelvin. - Apply Charles's Law to solve for the new volume \( V_2 \). - Present your answer rounded to 3 significant digits. ### Conversion of Temperatures: - Initial Temperature \( T_1 \): \( 6°C = 279 \, \text{K} \) - Final Temperature \( T_2 \): \( -31°C = 242 \, \text{K} \) ### Calculation: Given: \( V_1 = 37.5 \, \text{L} \), \( T_1 = 279 \, \text{K} \), \( T_2 = 242 \, \text{K} \) Using Charles's Law: \[ \frac{37.5}{279} = \frac{V_2}{242} \] Solve for \( V_2 \): \[ V_2 = \frac{37.5 \times 242}{279} \] ### New Volume \( V_2 \): Calculate the expression to find the approximate volume, rounding to 3 significant digits.
The vapor pressure of methanol at 25 °C is 126. torr. Calculate the vapor pressure in mmHg and atm. Round each of your answers to 3 significant digits.

Box for "mmHg" and "atm" values.

Button options include a checkmark, reset, and help.
Transcribed Image Text:The vapor pressure of methanol at 25 °C is 126. torr. Calculate the vapor pressure in mmHg and atm. Round each of your answers to 3 significant digits. Box for "mmHg" and "atm" values. Button options include a checkmark, reset, and help.
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