When the amount of work done is 333 cal and internal energy is 167 cal then heat supplied is _.
Correct answer: C. 500 cal
- A. 167 cal
- B. 175 cal
- C. 500 cal
- D. 600 cal
Explanation
By the first law of thermodynamics, the total energy of a system remains constant, and it can be converted from one form to another. It is given by the equation:ΔU = Q - Wwhere ΔU is the change in internal energy of the system, Q is the heat supplied to the system, and W is the work done by the system.Given:Work done (W) = 333 calChange in internal energy (ΔU) = 167 calSubstituting the values in the equation, we get:ΔU = Q - W167 = Q - 333Q = 167 + 333Q = 500 calTherefore, the heat supplied to the system is 500 cal. Answer is (c) 500 cal.
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About First Law of Thermodynamics
The first law relates heat supplied, work done and the change in internal energy through energy conservation. Problems use sign conventions and apply the law to isothermal, adiabatic, isobaric and isochoric processes. Internal energy is a state function, while heat and work depend on the path followed.
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