What is the change in entropy ($\Delta$ S) when two moles of silver (108 g/mole) is completely melted at 961$\degree$C? (The heat of fusion of silver is 8.82 *10⁴ J/kg.)

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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. First, convert the heat of fusion to J/mole: 8.82 x 10^4 J/kg * 108 g/mole * (1 kg/1000 g) = 9525.6 J/mole. For two moles, Q = 2 * 9525.6 J = 19051.2 J. Convert 961°C to Kelvin: 961 + 273.15 = 1234.15 K. ΔS = 19051.2 J / 1234.15 K = 15.4 J/K.

What Is the Change in Entropy Δ\DeltaΔ S) When Two Moles of Silver (108 G/mole) Is Completely

What Is the Change in Entropy $\Delta$ S) When Two Moles of Silver (108 G/mole) Is Completely