Question

17. State first law of thermodynamics. what conclusion do you draw from it
(a) for an isothermal Process
(b) for an adiabatic process.

Answer 1

Dear Student

First law of thermodynamics

Heat given to a system is equal to the sum of change in internal energy of the system and work done by the system.

The first law of thermodynamics states that the energy of an isolated system is constant.

ΔQ = ΔU + ΔW, is the mathematical statement of the first law of thermodynamics.

where ΔQ = heat given to the system

ΔU = the change in the internal energy of the system, which is dependent on the change in temperature during the process

ΔW = the work done by system.

It basically means that energy can neither be created nor be destroyed, although it can be converted from one form to another.

Now,

$$\begin{gathered} Forisothermal,∆T=0;\sin cetempertaureiscons\tan tfortheprocess. \\ Thus,∆U=0 \\ \Rightarrow ∆W=∆Q \\ Foradiabatic,∆Q=0;\sin cetheheatchangeiszerofortheprocess \\ \Rightarrow ∆W=-∆U \end{gathered}$$