Predict how the entropy of the system is affected in the following process. Alright, so for the first one, we have methane gas at 125℃ and it's transitioning to methane gas at 200℃. So the phase of method is still staying the same, but our temperature is increasing. Increasing our temperature would mean that our methane molecules can absorb that extra thermal energy, using it to propel themselves even more, becoming more chaotic, increasing their degrees of freedom. So here increasing temperature would cause an increase. It might change in entropy.
Alright. Next we have here potassium chlorate solid, and it's in a 7 liter container. And then we have potassium chlorate liquid in a three liter container, all right. So changing the volume of the container is a way of affecting the pressure in the container. Remember, there's an inverse relationship between pressure and volume. So our volume is going down from 3 liters to 7 liters, which would mean pressure is going up. But that's kind of a trick question here. Why? Because whether we're looking at what we're starting with and what we're ending, we're dealing with solids and liquids.
Solids and liquids are not going to be as affected by changes in pressure, at least not something as small as going from A7 litre container to a three liter container. So what you should really be looking at is the phase change we're going from solid potassium chlorate to liquid potassium chlorate. Liquids have more degrees of freedom. Their molecules are able to move around more. So because of this change in our phase, there's going to be an increase in the change in entropy. So again, entropy change is going up because we're going from a solid, which has less degrees of freedom, less entropy, to a liquid which has more degrees of freedom, more movement, more entropy.
Alright, So in both choices, the changing entropy is increasing.
