For the reaction NaCl(s)→waterNa+(aq)+Cl–(aq),ΔH=+1 kcal/mol (+4.184 kJ/mol)NaCl\left(s\right)\xrightarrow{water}$$Na^{+}$$\left(aq\$$right)+Cl^{–}$$\left(aq\right),\Delta H=\text{+1 kcal/mol (+4.184 kJ/mol)} b. Does entropy increase or decrease in this process?

Ch.7 Chemical Reactions: Energy, Rate and Equilibrium

McMurry - Fundamentals of General, Organic, and Biological Chemistry 8th Edition

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McMurry 8th Edition

Ch.7 Chemical Reactions: Energy, Rate and Equilibrium

문제 37b

7장, 문제 37b

For the reaction
$N a C l (s) \overset{w a t e r}{\to} N a^{+} (a q) + C l^{–} (a q), Δ H = +1 kcal/mol (+4.184 kJ/mol)$
b. Does entropy increase or decrease in this process?

검증된 단계별 안내

Step 1: Understand the reaction. The reaction shows the dissolution of solid sodium chloride (NaCl) into its ions, sodium (Na⁺) and chloride (Cl⁻), in water. This process involves breaking the ionic lattice of NaCl and dispersing the ions into the solution.

Step 2: Recall the concept of entropy (S). Entropy is a measure of the disorder or randomness in a system. Processes that increase the number of particles or the distribution of energy typically result in an increase in entropy.

Step 3: Analyze the change in the system. In this reaction, a single solid (NaCl) is converted into two separate ions (Na⁺ and Cl⁻) in an aqueous solution. The ions are free to move in the solution, which increases the randomness and disorder of the system.

Step 4: Consider the physical states. Solids have a more ordered structure compared to ions in solution. The transition from a solid to dissolved ions represents a significant increase in disorder.

Step 5: Conclude the entropy change. Since the process involves breaking a solid lattice and dispersing ions into a more disordered state, the entropy of the system increases during this reaction.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Entropy

Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it quantifies the number of ways a system can be arranged, with higher entropy indicating greater disorder. When a solid dissolves in a solvent, such as NaCl in water, the ions become more dispersed, typically leading to an increase in entropy.

Enthalpy Change (∆H)

Enthalpy change (∆H) refers to the heat absorbed or released during a chemical reaction at constant pressure. A positive ∆H, as in the case of NaCl dissolving in water, indicates that the process is endothermic, meaning it requires energy input. This energy is used to break the ionic bonds in the solid and to separate the ions in the solution.

Gibbs Free Energy (∆G)

Gibbs Free Energy (∆G) combines enthalpy and entropy to determine the spontaneity of a process. The relationship is given by the equation ∆G = ∆H - T∆S, where T is the temperature in Kelvin and ∆S is the change in entropy. A process is spontaneous if ∆G is negative, which can occur even if ∆H is positive, provided that the increase in entropy (∆S) is significant enough.

For the reaction NaCl(s)→waterNa+(aq)+Cl–(aq),ΔH=+1 kcal/mol (+4.184 kJ/mol)NaCl\(\left\)(s\(\right\))\(\xrightarrow{water}\)Na^{+}\(\left\)(aq\(\right\))+Cl^{–}\(\left\)(aq\(\right\)),\(\Delta\) H=\(\text{+1 kcal/mol (+4.184 kJ/mol)}\) b. Does entropy increase or decrease in this process?