what is the first law of thermodynamics in chemistry it is confusing at W and -W
Answers
Explanation:
The first law of thermodynamics is a version of the law of conservation of energy, adapted for thermodynamic processes, distinguishing two kinds of transfer of energy, as heat and as thermodynamic work, and relating them to a function of a body's state, called Internal energy.
The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but can be neither created nor destroyed.
For a thermodynamic process without transfer of matter, the first law is often formulated[1][nb 1]
{\displaystyle \Delta U=Q-W}{\displaystyle \Delta U=Q-W},
where ΔU denotes the change in the internal energy of a closed system, Q denotes the quantity of energy supplied to the system as heat, and W denotes the amount of thermodynamic work done by the system on its surroundings. An equivalent statement is that perpetual motion machines of the first kind are impossible.
For processes that include transfer of matter, a further statement is needed: 'With due account of the respective reference states of the systems, when two systems, which may be of different chemical compositions, initially separated only by an impermeable wall, and otherwise isolated, are combined into a new system by the thermodynamic operation of removal of the wall, then
{\displaystyle U_{0}=U_{1}+U_{2}}{\displaystyle U_{0}=U_{1}+U_{2}},
where U0 denotes the internal energy of the combined system, and U1 and U2 denote the internal energies of the respective separated systems.'
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Answer:
The first law of thermodynamics, also known as Law of Conservation of Energy, states that energy can neither be created nor destroyed; energy can only be transferred or changed from one form to another.
Formula
U = Q - W
U = change in internal energy
Q = heat added
W = work done by the system
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