[rurayhan]

This is one single problem with multiple parts

1) Consider the melting of 2.00 moles of liquid water at 0.0C in an isolated box whose temperature is held at 25 C. ( Delta H fusion for H20 is 6.01 kj/mol) Note Delta H fusion refers to ice melting.

a) What is the Delta S water for this process?
b) What is the delta S box for this process?
c) what is the total entropy change for the process?
d) IS the melting of water at this temperature a spontanous or nonspontanous process? explain.

Now, I am just not posting it, I have actually tried this problem, but I feel as if my knowledge regarding this problem is inadequete. For part A i decided to do Delta H fusion times 2 moles / 25 +278 K to find the entropy. Since ice melting is an endothermic process ..However I am still questioning my  methods on part  A and B and so on.

Hopefully somone can answer this problem.



- rurayhan

[Yggdrasil]

a)  Since entropy is a state function (meaning its value is path-independent), the best way to determine ΔS_system is to construct a reversible path between the two states and calculate the ΔS_sys for the reversible path.

b)  Since the box is the surroundings, you just use the formula ΔS_surroundings = q/T