객관식
Which sample has the highest entropy under the stated conditions?
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19. Chemical Thermodynamics
Entropy
객관식
Predict the sign of ∆S in the system for each of the following processes:
a) Ag+ (aq) + Br - (aq) → AgBr (s)
b) CI2 (g) → 2 CI - (g)
c) CaCO3 (s) → CaO (s) + CO2 (g)
d) Pb (s) at 50°C → Pb (s) at 70°C
A
a) ∆S = + b) ∆S = + c) ∆S = + d) ∆S = +
B
a) ∆S = - b) ∆S = + c) ∆S = - d) ∆S = +
C
a) ∆S = - b) ∆S = + c) ∆S = - d) ∆S = -
D
a) ∆S = - b) ∆S = + c) ∆S = + d) ∆S = +
검증된 단계별 안내1
Step 1: Understand that entropy (∆S) is a measure of disorder or randomness in a system. An increase in disorder results in a positive ∆S, while a decrease in disorder results in a negative ∆S.
Step 2: Analyze process (a): Ag+ (aq) + Br- (aq) → AgBr (s). Here, two aqueous ions combine to form a solid. This process decreases the disorder as the ions are more ordered in the solid state, so ∆S is negative.
Step 3: Analyze process (b): Cl2 (g) → 2 Cl- (g). A diatomic molecule is dissociating into two separate atoms, increasing the number of gas particles and thus increasing disorder. Therefore, ∆S is positive.
Step 4: Analyze process (c): CaCO3 (s) → CaO (s) + CO2 (g). A solid decomposes into another solid and a gas. The formation of a gas increases the disorder, so ∆S is positive.
Step 5: Analyze process (d): Pb (s) at 50°C → Pb (s) at 70°C. The temperature increase causes the solid's particles to move more vigorously, increasing disorder. Thus, ∆S is positive.
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