If heat given is 6 kcal and work done is 6 kJ, then internal energy is _.
Correct answer: A. 19.1 kJ
- A. 19.1 kJ
- B. 25.2 kJ
- C. 25 kJ
- D. Zero
Explanation
Correct Option:ATo determine the internal energy, we need to apply the First Law of Thermodynamics, which states that the change in internal energy (ΔU) is equal to the heat added (Q) minus the work done (W) on the system.ΔU = Q - WGiven that the heat given (Q) is 6 kcal and the work done (W) is 6 kJ, we need to convert the units to ensure consistency:1 kcal = 4.184 kJConverting the heat given to kJ:6 kcal * (4.184 kJ/1 kcal) = 25.104 kJNow, we can substitute the values into the equation:ΔU = 25.104 kJ - 6 kJ= 19.104 kJ
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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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