Statement-I Heat and work are ''definite quantities''.
Statement-II Heat and work are not properties of a system. Their values depend on the path of the process and vary accordingly.

Options

A. If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
B. If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To analyze the given statements and determine their validity, we can follow these steps:

### Step 1: Understand the Definitions
- **Heat and Work**: In thermodynamics, heat and work are forms of energy transfer. They are not stored within the system but are exchanged between the system and its surroundings.
- **Definite Quantities**: These are quantities that do not depend on the path taken to achieve a particular state. They are typically associated with state functions (like internal energy, enthalpy, etc.).

### Step 2: Analyze Statement I
- **Statement I**: "Heat and work are 'definite quantities'."
- This statement is **incorrect**. Heat and work are not definite quantities; they are path-dependent. Their values can change based on the process taken to transfer energy.

### Step 3: Analyze Statement II
- **Statement II**: "Heat and work are not properties of a system. Their values depend on the path of the process and vary accordingly."
- This statement is **correct**. Heat and work are indeed not properties of a system. They depend on the specific path taken during a process, which means their values can vary.

### Step 4: Conclusion
- Since Statement I is false and Statement II is true, we conclude that:
- Statement I is incorrect.
- Statement II is correct.

### Final Answer
- The correct answer is that Statement I is false, and Statement II is true.