Final answer:
The heat lost when 75g of water vapor cools from 393 K to 263 K involves the heat released during condensation plus the heat lost when the condensed water cools to the final temperature. However, the calculated heat loss exceeds the highest option provided, indicating a potential error in the question or the answer choices.
Step-by-step explanation:
To calculate the amount of heat lost when 75g of water vapor cools from 393 K to 263 K, we need to account for the energy change during the phase change from vapor to liquid (condensation) and the subsequent cooling of the condensed water to the final temperature. Using the heat of vaporization of water, which is approximately 2,250 J/g, we first calculate the heat released during condensation. For cooling the liquid water from 100°C (373 K) to the final temperature, we use the specific heat capacity of water, which is 4.18 J/g/°C.
The process is as follows:
- Calculate the heat released during the condensation of 75g of water vapor at 100°C (373 K).
- Calculate the heat lost when the condensed water cools from 100°C to -10°C (263 K).
Heat lost during condensation = mass × heat of vaporization
Heat lost = 75g × 2,250 J/g = 168,750 J
However, as the question only supplies options up to 25,000 J, it seems there might be a misunderstanding in the question or the given options. The calculated value is not within the provided options.