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When ice melts at 1^(@)C : (a)an incre...

When ice melts at `1^(@)C` :
(a)an increase in entropy
(b)a decrease in enthalpy
(c)a decrease in free energy
(d)process is spontaneous

A

an increase in entropy

B

a decrease in enthalpy

C

a decrease in free energy

D

process is spontaneous

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the melting of ice at 1°C, we will analyze each option based on thermodynamic principles. ### Step-by-Step Solution: 1. **Understanding the Process**: - When ice melts at 1°C, it transitions from a solid state (ice) to a liquid state (water). This process involves the absorption of heat (latent heat of fusion) and is a phase change. 2. **Entropy Change**: - Entropy (S) is a measure of the disorder or randomness in a system. - In the solid state (ice), the molecules are arranged in a fixed, orderly structure. When ice melts, the molecules gain energy and move into a more disordered liquid state. - Therefore, the entropy increases during the melting process. - **Conclusion**: The statement about an increase in entropy is correct. 3. **Enthalpy Change**: - Enthalpy (H) is a measure of the total energy of a thermodynamic system. - When ice melts, it absorbs heat, which means the enthalpy of the system increases (not decreases). - **Conclusion**: The statement about a decrease in enthalpy is incorrect. 4. **Gibbs Free Energy Change**: - Gibbs free energy (G) is defined as G = H - TS, where T is the temperature in Kelvin and S is the entropy. - For a process to be spontaneous, the change in Gibbs free energy (ΔG) must be negative. - Since the entropy increases (ΔS > 0) and the process occurs at a constant temperature, the term -TΔS becomes more negative, which can lead to a decrease in ΔG. - **Conclusion**: The statement about a decrease in free energy is correct. 5. **Spontaneity of the Process**: - A process is spontaneous if ΔG < 0 and ΔS > 0. - Since both conditions are satisfied during the melting of ice at 1°C, the process is indeed spontaneous. - **Conclusion**: The statement that the process is spontaneous is correct. ### Summary of Answers: - (a) An increase in entropy: **Correct** - (b) A decrease in enthalpy: **Incorrect** - (c) A decrease in free energy: **Correct** - (d) Process is spontaneous: **Correct** ### Final Answer: The correct statements are (a), (c), and (d).
To solve the question regarding the melting of ice at 1°C, we will analyze each option based on thermodynamic principles. ### Step-by-Step Solution: 1. **Understanding the Process**: - When ice melts at 1°C, it transitions from a solid state (ice) to a liquid state (water). This process involves the absorption of heat (latent heat of fusion) and is a phase change. 2. **Entropy Change**: ...
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