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I know that the change in internal energy is equal to q+w (the first law of thermodynamics). Where does temperature come into play with this (specifically regarding isothermal processes)? How come when the change in internal energy is zero, the change in temperature is also zero, but work and heat have values other than zero?
Isothermal processes are processes at a constant temperature throughout the whole process so the temperature remains the same at the end. This would mean that the change in temperature would be the same values subtracting from each other which would equate to 0. Furthermore, the kinetic energy and potential energy of the process remains the same therefore the change in internal energy would also be equal to 0.
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