This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.
ScanSolve AI Answer
Here's how to calculate the increase in entropy: To find the increase in entropy ( S) during a phase change at constant temperature, we use the formula: S = (Q)/(T) where Q is the heat absorbed and T is the absolute temperature in Kelvin. For melting, the heat absorbed (Q) is given by: Q = mL_f where m is the mass and L_f is the latent heat of fusion. Given values: • Mass of ice, m = 1.00 kg • Temperature, T_C = 0^ C • Latent heat of fusion of water, L_f = 334 × 10^3 J/kg (standard value) Step 1: Convert the temperature from Celsius to Kelvin. T_K = T_C + 273.15 T_K = 0 + 273.15 = 273.15 K Step 2: Calculate the heat absorbed (Q) to melt the ice. Q = mL_f Q = (1.00 kg) × (334 × 10^3 J/kg) Q = 334 × 10^3 J Step 3: Calculate the increase in entropy ( S). S = (Q)/(T_K) S = 334 × 10^3 J273.15 K S ≈ 1222.84 J/K S = 1223 J/K What's next? Send 'em!