Answer:
Total energy decreases as well as total entropy.
Explanation:
Hello,
In this case, due to the effect of the high water's temperature, the ice will probably melt or at least, will decrease its initial temperature. In such a way, since no heat is exchanged with the surroundings, the system's equilibrium energy will be between the initial hot water's energy and the initial ice's energy, in other words, the total energy will decrease if the hot water's energy is larger than the ice's energy based on the first law of thermodynamics. Moreover, the total entropy of the system will decrease as long as during the aforesaid cooling process, the arrangement of system becomes less disordered (or more ordered) which is related with an entropy decrease, based on the second law of thermodynamics.
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The total energy and the total entropy in the system reduces as the system reaches equilibrium.
Entropy is the degree of disorderliness in a system.
Entropy increases with temperature and vice versa.
Enthalpy is the sum total of the internal energy or heat content in a system.
The enthalpy of a system increases with temperature.
When ice is added to the system and allow to melt, the temperature of the system at equilibrium decreases as heat in used to melt the ice, thus, the energy and entropy of the system decreases.
Learn more about b and entropy at: https://brainly.com/question/24376583
