Recall that work (w) is given by:
• (+): heat, q is gained by the system (i.e. endothermic rxn )
• (–): heat, q is released by the system (i.e. exothermic rxn)
• (+): work is done by the surroundings to the system (compression)
• (–): work is done by the system to the surroundings (expansion)
At constant P → q = ΔH (enthalpy)
At constant V → w = 0
Imagine a container placed in a tub of water, as depicted in the accompanying diagram.
If neither the volume nor the pressure of the system changes during the process, how is the change in internal energy related to the change in enthalpy?
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