l1. A weather balloon is filled with 16.0 L of helium at a temperature of26°C an...

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October 2022 1 4 Report

l1. A weather balloon is filled with 16.0 L of helium at a temperature of
26°C and a pressure of 700 mm Hg. What is the pressure of the
helium in the balloon in the upper atmosphere when the temperature
is -33°C and the volume becomes 35.0L?

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GreatRedSpot

SOLUTION:

Step 1: List the given values.

To convert the temperature from degree Celsius to kelvin, add 273 to the temperature expressed in degree Celsius.

$\begin{aligned} & P_1 = \text{700 mmHg} \\ & V_1 = \text{16.0 L} \\ & T_1 = 26^{\circ}\text{C} = \text{299 K} \\ & V_2 = \text{35.0 L} \\ & T_2 = -33^{\circ}\text{C} = \text{240 K} \end{aligned}$

Step 2: Calculate the final pressure using combined gas law.

$\begin{aligned} P_2 & = \frac{P_1V_1T_2}{V_2T_1} \\ & = \frac{(\text{700 mmHg})(\text{16.0 L})(\text{240 K})}{(\text{35.0 L})(\text{299 K})} \\ & = \boxed{\text{257 mmHg}} \end{aligned}$

Hence, the pressure of helium in the balloon is 257 mmHg.

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