Help with entropy change question

[justinbaker]

So I am studying for finals and this is on the set of questions that our teacher told us to review.

http://imageserver4.textamerica.com/user.images.x/98/IMG_372198/_0509/T520060509170033508.jpg

so not even quite sure how to attack this one, so any help would be great, thanks

 

[lightgrav]

Is Energy conserved in the system? That is, are the two subsystems able to exchange Energy with the "outside"?

I would presume that neither box changes its Volume as it warms or cools ...
the alternative would be to presume that they maintain equal pressure,
but pressure is not mentioned (except that an "ideal gas" has PV=NkT).

 

[kyle8921]

Entropy change is a measure of the disorder or randomness in a system. It is often denoted by the symbol ΔS (delta S) and can be calculated using the equation ΔS = Q/T, where Q is the heat added or removed from the system and T is the temperature in Kelvin.

In the image provided, it appears to be a question asking about the entropy change for a specific chemical reaction. To approach this question, you will need to know the specific heat capacity of each substance involved, as well as the temperature change during the reaction. From there, you can use the equation ΔS = Q/T to calculate the entropy change for each substance, and then determine the overall entropy change for the reaction by adding or subtracting the individual values.

It may also be helpful to consider the physical state (solid, liquid, gas) of each substance and how that may affect the entropy change. Generally, the more disordered a substance is, the higher its entropy change will be.

I hope this helps and good luck on your finals! Remember to always check your units and make sure they are consistent throughout your calculations.