Import Question JSON

$\text{Hint: Temperature increases, entropy also increases.}$ $\text{To determine which process has a negative entropy change, we need to analyze each option based on principles of entropy:}$ $\text{1. Bromine (l)}\rightarrow\text{Bromine(g):}$ $\text{This represents a phase change from liquid to gas. The gaseous phase has more disorder and freedom of movement than the liquid phase. Therefore,}$ $\Delta\text{S is positive for this process.}$ $\text{2. C(s) + H}_2\text{O(g)} \rightarrow\text{CO(g) + H}_2\text{(g):}$ $\text{Here we have 1 solid and 1 gas molecule converting to 2 gas molecules. Since gases have higher entropy than solids, and we end up with more gas molecules, the disorder increases. Therefore,}$ $\Delta\text{S is positive for this reaction.}$ $\text{3. N}_2\text{(g,10 atm)}\rightarrow\text{N}_2\text{(g,1 atm):}$ $\text{This represents a decrease in pressure for a gas. When pressure decreases, gas molecules have more available space and greater freedom of movement, which increases disorder. Therefore,}$ $\Delta\text{S is positive for this process.}$ $\text{4. Fe (1mol, 400 K)} \rightarrow \text{Fe(1mol, 300 K):}$ $\text{This represents a decrease in temperature of iron from 400 K to 300 K. When temperature decreases, molecular motion decreases, leading to less disorder in the system. Therefore,}$ $\Delta\text{S is negative for this process.}$ $\text{Based on the analysis, only option 4 shows a negative entropy change, as a decrease in temperature leads to decreased molecular motion and disorder.}$