application$)$ Calculate the change in entropy $()$ for the following processes:a$)$ Heating $0\mathrm{.}5$ kg of solid ice from $100\backslash$deg C to $0\backslash$deg C$.$b$)$ Freezing $0\mathrm{.}5$ kg of liquid water at $0\backslash$deg C to solid ice at $0\backslash$deg C$.$c$)$ Cooling $0\mathrm{.}5$ kg of liquid water from $100\backslash$deg C to $0\backslash$deg C$.$d$)$ Vaporizing $0\mathrm{.}5$ kg of liquid water at $100\backslash$deg C to steam at $100\backslash$deg C$.$e$)$ Which one of the two phase transitions $($freezing or vaporizing$)$ has the larger magnitude in thechange of entropy? Explain in terms of the statistical model of entropy.f$)$ For each process a$)-$d$)$ does the entropy of the environment change? If so$,$ does it increase ordecrease? How do you know?