calculate the change in internal energy of system if 500J of work is done by the system and 0.5kj of heat is absorbed by the system from the surroundings?
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The First Law of Thermodynamics states that energy can be converted from one form to another with the interaction of heat, work and internal energy, but it cannot be created nor destroyed, under any circumstances. Mathematically, this is represented as
ΔH=ΔU+ΔnRT
where,
ΔH is the heat exchanged between a system and its surroundings,
ΔU is the total change in internal energy of a system,
ΔnRT is the work done by or on the system.
Given,
ΔH=2Kcal=8400JW=500JSo,ΔU=8400−500=7900J.
Hence,option A is correct.
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