Answer:
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Explanation:
To calculate the pressure change when a gas is cooled at constant volume, you can use the ideal gas law:
\[ P_1/T_1 = P_2/T_2 \]
where:
- \( P_1 \) is the initial pressure,
- \( T_1 \) is the initial temperature,
- \( P_2 \) is the final pressure,
- \( T_2 \) is the final temperature.
Given that the volume is constant, \( V_1 = V_2 \), and you can simplify the equation to:
\[ \frac{P_1}{T_1} = \frac{P_2}{T_2} \]
Now, plug in the values:
\[ \frac{P_1}{343 \, \text{K}} = \frac{P_2}{283.15 \, \text{K}} \]
Solve for \( P_2 \):
\[ P_2 = P_1 \times \frac{283.15 \, \text{K}}{343 \, \text{K}} \]
Assuming you have the initial pressure \( P_1 \), you can substitute that value to find \( P_2 \).
