Question

What is the decrease in entropy of 25.0 g of water that condenses on a bathroom mirror at a temperature of 35.0º C, assuming no change in temperature and given the latent heat of vaporization to be 2450 kJ/kg?

a) -5.0 J/K
b) -7.5 J/K
c) -10.0 J/K
d) -12.5 J/K

Answer 1

The decrease in entropy of 25.0 g of water condensing on a bathroom mirror at a constant temperature of 35.0° C can be calculated using the formula ΔS = Q/T. Since the temperature remains constant, the change in entropy is equivalent to the heat transferred. The heat transferred can be found using the formula Q = mL, where Q is the heat transferred, m is the mass of the water, and L is the latent heat of vaporization. Plugging in the values, the decrease in entropy is 61.25 J.

Step-by-step explanation:

The decrease in entropy of water that condenses on a bathroom mirror can be calculated using the formula ΔS = Q/T, where ΔS is the change in entropy, Q is the heat transferred, and T is the temperature. Since the temperature remains constant, the change in entropy is equivalent to the heat transferred.

The heat transferred can be found using the formula Q = mL, where Q is the heat transferred, m is the mass of the water, and L is the latent heat of vaporization. Plugging in the values, we have Q = (0.025 kg)(2450 kJ/kg) = 61.25 J.

Therefore, the decrease in entropy of the water is 61.25 J.