Question

Assertion A: If \( dQ \) and \( dW \) represent the heat supplied to the system and the work done on the system respectively, then according to the first law of thermodynamics: \[ dQ = dU - dW. \]
Reason R: First law of thermodynamics is based on the law of conservation of energy.
In the light of the above statements, choose the correct answer from the options given below:

• A. Both A and R are correct and R is the correct explanation of A
• B. A is correct but R is not correct
• C. A is not correct but R is correct
• D. Both A and R are correct but R is not the correct explanation of A

Hint:

For assertion-reason questions:
• Ensure the statement and reasoning align with the fundamental laws.
• Validate whether the reason provides a logical explanation for the assertion.

Answer 1

The Correct Option is A

• The first law of thermodynamics states: \[ \Delta Q = \Delta U + \Delta W. \]
• Rearranging gives: \[ dQ = dU - dW. \]
• This law is based on the conservation of energy.

Final Answer: \( \boxed{(Option 1)} \)

Answer 2

∆Q = heat supplied to system
∆W = work done on the system 
∴ ∆U = ∆Q – ∆W 
This comes from conservation of energy.