Answer :
Final answer:
Using Charles's Law and the given conditions, the final volume of the 2.00-mole sample of N2 gas law when it is heated from 0°C to 170°C at a constant pressure is found to be approximately 72.8 L. None of the provided answer options are correct.
Explanation:
In this question, we are working with aspects of the ideal gas law and specifically, Charles's Law which states that for an ideal gas at constant pressure, the volume is directly proportional to the absolute temperature. From the standard conditions of temperature and pressure (STP), we know that one mole of an ideal gas at STP has a volume of about 22.4 L. Hence, a 2.00-mole sample of N2 gas at 0°C (273.15 K) would occupy a volume of 44.8 L.
When the gas is heated from 273.15 K to 170°C (443.15 K), its volume should increase proportionally. Using Charles's Law (V1/T1 = V2/T2), and solving for the unknown final volume, we find: V2 = (V1/T1) * T2 = (44.8 L / 273.15 K) * 443.15 K ≈ 72.8 L. Hence, none of the options listed in your question is correct.
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