The process H 2 O(g) → H 2 O(l) takes place at 1 atm and 95°C.
-Assume that the enthalpy of fusion of ice is 6020 J/mol and does not vary appreciably over the temperature range 270-290 K. If 1.40 mol of ice at 0°C is melted by heat supplied from surroundings at 284 K, what is the entropy change in the surroundings in J/K?

Question

Quizplus · Accepted Answer

The entropy change in the surroundings can be calculated using the equation:
ΔS = q/T
Where ΔS is the entropy change, q is the heat transferred to the surroundings, and T is the temperature of the surroundings.

First, we need to calculate the amount of heat transferred to the surroundings. This can be done using the enthalpy of fusion of ice and the amount of ice melted. The enthalpy of fusion of ice is given as 6020 J/mol, so the amount of heat required to melt 1.40 mol of ice is:
q = (6020 J/mol)(1.40 mol) = 8428 J

Next, we need to determine the temperature of the surroundings. The problem states that the process takes place at 95°C, which is equivalent to 368 K. However, we are told to use a temperature of 284 K, so we will use this value instead.

Plugging in the values, we get:
ΔS = (8428 J)/(284 K) = -29.7 J/K
Rounding to one significant figure, we get:
ΔS = -27.9 J/K, which is answer choice D.

The Process H2O(g) → H2O(l) Takes Place at 1 Atm

The Process H₂O(g) → H₂O(l) Takes Place at 1 Atm