Answer:
C is correct
Explanation:
The given reaction is the formation of ammonia from nitrogen and hydrogen:
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \]
Let's analyze each statement:
A. **ΔSsys is negative:** This statement is likely false. The reaction involves the formation of a more disordered (higher entropy) product from less disordered (lower entropy) reactants, suggesting an increase in entropy for the system. Therefore, ΔSsys is likely positive.
B. **ΔHsys is positive:** This statement is also likely false. The formation of ammonia is an exothermic reaction, meaning it releases heat. Therefore, ΔHsys is negative.
C. **ΔSsurr is negative:** This statement is true. Since the reaction releases heat (ΔHsys is negative), the surroundings gain heat, leading to an increase in entropy for the surroundings, making ΔSsurr negative.
D. **ΔUniv is negative:** This statement is true. Since the reaction releases heat and has a positive entropy change for the system, ΔUniv (the total entropy change of the universe) is likely negative, as the increase in entropy of the surroundings is not enough to compensate for the decrease in entropy of the system.
So, the correct answer is:
C. ΔSsurr is negative.