Ice cubes at 0 C are poured into a glass that initially contains 150 g of liquid water at 20 C. The contents of the glass are gently stirred stirred and after a short time some of the ice melts and the liquid cools to 0 C. No apppreciable heat exchange with the environment takes place during this process.

(a) Calculate the entropy change of the universe during the process. Use only the following data (no external data sources): The heat capacity of liquid water is 4.18 J/g*K, which you may assume to be independent of temperature over the range of interest. For liquids, Cp=Cv)

(b) If the same process were performed reversibly, how much useful work would be obtained from it. Any required heat exchange to achieve the same final state reversibly should be with the environment at 20 C.

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.

definition

                    entropy is a measure of the randomness or the extent of disorder of a chemical process.

                      enthalpy is a measure of the heat change of a reaction occurring at a constant pressure.

measurement units:

                        entropy is measured in joule per kelvin (jk⁻¹)   whereas enthalpy is measured in joule per mole (jmol⁻¹)

requirements:

                            entropy has no requirements or limits, and its change is measured by the division between the heat change of the chemical process and the temperature.

                              in contrast, enthalpy can only be related to the heat change of the reaction under standard conditions.

yes

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