2.20 kilograms of water at 1.00 atm at the boiling point of 100°C is heated until all the water vaporizes.What is its change in entropy? (For water,L_v = 2.26 × 10⁶ J/kg) A)2.67E+4 J/K B)1.33E+4 J/K C)6.66E+3 J/K D)4.44E+3 J/K E)1.82E+4 J/K

Question

Quizplus · Accepted Answer

The change in entropy (ΔS) is calculated using the formula ΔS = Q/T, where Q is the heat absorbed and T is the temperature in Kelvin. Q = mass × L_v = 2.20 kg × 2.26 × 10^6 J/kg = 4.972 × 10^6 J. T = 100°C = 373 K. ΔS = 4.972 × 10^6 J / 373 K = 1.33 × 10^4 J/K.

220 Kilograms of Water at 1