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Statement 1 : Entropy of solution is les...

Statement 1 : Entropy of solution is less than entropy of pure solvent.
Statement 2 : The freezing point of water is depressed by the addition of glucose.

A

Statement 1 is true, statement 2 is true, statement 2 is a correct explanation for statement 1

B

Statement 1 is true, statement 2 is true , statement 2 is not a correct explanation for statement 1

C

Statement 1 is true, statement 2 is false

D

Statement 1 is false, statement 2 is true

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the given statements, we will evaluate each one based on the principles of thermodynamics and colligative properties. ### Step-by-Step Solution: **Step 1: Evaluate Statement 1** - **Statement 1**: "Entropy of solution is less than entropy of pure solvent." - **Analysis**: Entropy is a measure of disorder or randomness in a system. When a solute is added to a solvent to form a solution, the overall disorder of the system increases. This is because the solute particles disrupt the orderly arrangement of the solvent molecules, leading to an increase in entropy. Therefore, the entropy of the solution is greater than that of the pure solvent. - **Conclusion**: Statement 1 is **False**. **Step 2: Evaluate Statement 2** - **Statement 2**: "The freezing point of water is depressed by the addition of glucose." - **Analysis**: This statement refers to a colligative property of solutions. When a non-volatile solute, such as glucose, is added to a solvent like water, it lowers the freezing point of the solvent. This phenomenon is known as freezing point depression. The presence of solute particles interferes with the formation of the solid structure of ice, thus lowering the temperature at which freezing occurs. - **Conclusion**: Statement 2 is **True**. **Final Conclusion**: - Statement 1 is False. - Statement 2 is True. - Therefore, the correct answer is option D: Statement 1 is false and Statement 2 is true.
To analyze the given statements, we will evaluate each one based on the principles of thermodynamics and colligative properties. ### Step-by-Step Solution: **Step 1: Evaluate Statement 1** - **Statement 1**: "Entropy of solution is less than entropy of pure solvent." - **Analysis**: Entropy is a measure of disorder or randomness in a system. When a solute is added to a solvent to form a solution, the overall disorder of the system increases. This is because the solute particles disrupt the orderly arrangement of the solvent molecules, leading to an increase in entropy. Therefore, the entropy of the solution is greater than that of the pure solvent. - **Conclusion**: Statement 1 is **False**. ...
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