What is the decrease in entropy of \( 46.6 \mathrm{~g} \) of water that condenses on a bathroom mirror at a temperature of \( 30.4^{\circ} \mathrm{C} \), assuming no change in temperature and given the latent heat of vaporization to be \( 2450 \mathrm{~kJ} / \mathrm{kg} \) ? Select the correct answer \( 376 \mathrm{~J} / \mathrm{K} \) \( 199 \mathrm{~J} / \mathrm{K} \) \( 234 \mathrm{~J} / \mathrm{K} \) \( 173 \mathrm{~J} / \mathrm{K} \) \( 280 \mathrm{~J} / \mathrm{K} \)
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Since the latent heat of vaporization is given in kJ/kg, we need to convert the mass of water from grams to kilograms for consistency in units. \[ 46.6 \text{ g} = \frac{46.6}{1000} \text{ kg} = 0.0466 \text{ kg} \] Show more…
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