Question

8. At its melting point, 0°C, the heat of fusion of water is 1,435Kcal/mol. What is the molar entropy change for the melting of ice at 0°C? (A). 113.0cal/molK (B). 5.26cal/molk (C). 100 cal/molK. (D) 52.6 cal/molk​

Answer 1

the molar entropy change for the melting of ice at 0°C is 5.26 cal/molK. The answer is (B).

Step-by-step explanation:

The molar entropy change for the melting of ice can be calculated using the formula:

ΔSm = ΔHfus / T

where ΔHfus is the heat of fusion and T is the melting point temperature. In this case, ΔHfus = 1,435 Kcal/mol and T = 273 K (0°C + 273.15).

Substituting these values into the formula, we get:

ΔSm = (1,435 Kcal/mol) / 273 K

ΔSm = 5.26 cal/molK

Therefore, the molar entropy change for the melting of ice at 0°C is 5.26 cal/molK. The answer is (B).