Consider a very long, thin $1\mathrm{.}45-$kg cylinder of copper at a temperature $20\mathrm{.}0$ C$.$ The radius of the cylinder is $5\mathrm{.}00$ mm and the length is $2\mathrm{.}075$ m$.$ The specific heat of copper is $387$ J$/($kg$$C$).$ The thermal coefficient of linear expansion is $17106($C$)1.$ In the next part, this copper cylinder is removed from the oven and placed in a container with $4\mathrm{.}00$ kg of water that is already at a temperature of $93\mathrm{.}0$C$.$ The water warms to boiling temperature and part of it evaporates. How much energy is absorbed by the water as its temperature increases to $100$C$?$ What is the mass of water that evaporates before it comes to equilibrium with the copper?