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Answer :
Final answer:
This physics question requires the application of the Ideal Gas Law to calculate the final pressure of oxygen gas undergoing a compression and temperature change. By substituring the given volume and temperature values and solving for the unknown final pressure, an estimation can be made.
Explanation:
Applying the Ideal Gas Law
Your question revolves around the behaviors of gases under varying pressure, volume, and temperature conditions, which is commonly explained using the Ideal Gas Law formula: PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
Since the amount of gas (oxygen) is constant and the gas constant, R, is always the same, we can express the relationship of the rest variables in two situations P1V1/T1 = P2V2/T2.
Consequently, we can calculate the final pressure after the compression and temperature change. Just remember to convert all the temperature values to Kelvin format (K = °C + 273.15).
However, this application assumes the gas behavior is perfect, which isn't always the truth in real-world situations, but it should serve to provide a good estimation.
Learn more about Ideal Gas Law here:
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The complete question is: 62.5 L of oxygen at 18.0°C and an absolute pressure of 1.85 atm are compressed to 38.8 L, and at the same time, the temperature is raised to 56.0°C. is:
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