Calculate the entropy change, $S,$ when $1\mathrm{.}0kg$ of water is reversibly heated at constant pressure and in its initial state the water is as a block of ice at $T_0=-10C$ and in its final state it is as steam. at $T_f=200C$

To do this, use the fundamental definition of entropy $dS=\frac{d{Q}_{\text{r}\text{e}\text{v}}}{T}$

The specific heats at constant $P$ of ice, liquid water and vapor are $2\mathrm{.}090K\frac{J}{K}g,4\mathrm{.}184K\frac{J}{K}g$ and $2,259\mathrm{.}36K\frac{J}{K}g,$ respectively. The latent heat of a phase transition is the heat necessary for said phase transition to take place, and for the fusion transition, solid to liquid, it is $333\mathrm{.}5K\frac{J}{K}g,$ and the latent heat of vaporization is $2,257K\frac{J}{K}g.$