During winters, moisture condenses in the form of dew and can be seen on plant leaves and grass. The entropy of the system in such cases decreases as liquids process lesser disorder as compared to gases. With reference to the second law, which statement is correct. for the above process?

Options

A. The randomness of the universe decreases
B. The randomness of the surrounding decreases
C. Increase is randomness of surroundings equal the decrease in randomness of system
D. The increase in randomness of the surroundings is greater as compared to the decrease in randomness of the system

Explanation

To analyze the process of moisture condensing into dew on plant leaves and grass during winter, we can follow these steps:

### Step 1: Understand the Process
Moisture in the air (water vapor) condenses into liquid water (dew) when the temperature drops. This transition occurs from a gaseous state to a liquid state.

**Hint:** Identify the states of matter involved in the process (gas to liquid).

### Step 2: Analyze Entropy Changes
Entropy is a measure of disorder or randomness in a system. Gases have higher entropy compared to liquids because gas molecules are more dispersed and have more freedom of movement. Therefore, when water vapor condenses into liquid, the entropy of the system (the water itself) decreases.

**Hint:** Recall that gases have higher entropy than liquids.

### Step 3: Apply the Second Law of Thermodynamics
The second law states that the total entropy of an isolated system can never decrease over time. While the entropy of the system (water vapor condensing) decreases, the surroundings (the environment) experience an increase in entropy due to the release of heat during condensation.

**Hint:** Consider the overall entropy change in the universe, which includes both the system and surroundings.

### Step 4: Compare Entropy Changes
Although the system's entropy decreases, the surroundings' entropy increases significantly due to the heat released during the condensation process. The increase in entropy of the surroundings is greater than the decrease in entropy of the system.

**Hint:** Think about how energy transfer affects the surroundings.

### Step 5: Conclusion
Since the total entropy change (system + surroundings) must be positive according to the second law, we conclude that the process is spontaneous. Therefore, the correct statement regarding the process is that the increase in randomness (entropy) of the surroundings is greater than the decrease in randomness of the system.

**Hint:** Look for statements that reflect the overall increase in entropy in the universe.

### Final Answer
The correct statement is: "The increase in randomness of the surroundings is greater compared to the decrease in randomness of the system."

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