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Answer :
Answer: C
Explanation:
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Final answer:
The pressure in a refrigeration system charged with nitrogen is expected to decrease proportionally to the temperature decrease, assuming no nitrogen escaped the system. This can be shown using Gay-Lussac's law, a version of the Ideal Gas Law for constant volume conditions.
Explanation:
The student is asking about the relationship between temperature and pressure in a sealed refrigeration system when nitrogen was used to charge the system. This is related to the Ideal Gas Law that establishes a direct proportional relationship between pressure (P) and temperature (T) when the volume (V) and quantity (n) of gas are constant. We use Gay-Lussac's law, which is a form of the Ideal Gas Law when determining pressure changes at constant volume.
To calculate the expected pressure after the temperature drop without any nitrogen escaping from the system, we would use the formula:
P1/T1 = P2/T2,
where P1 is the initial pressure, T1 is the initial temperature in Kelvin, P2 is the final pressure, and T2 is the final temperature in Kelvin. Using this formula, we can deduce that if the temperature decreases and no nitrogen escaped, the pressure in the system would also decrease proportionally.
Since we are considering the Fahrenheit scale for temperature, we would first need to convert these temperatures to Kelvin before applying the formula. Here's how to convert Fahrenheit to Kelvin: K = (F - 32) * (5/9) + 273.15. Thus, the initial temperature of 75 degrees Fahrenheit is (75 - 32) * (5/9) + 273.15 K, and the final temperature of 50 degrees Fahrenheit is (50 - 32) * (5/9) + 273.15 K.
