A $0\mathrm{.}83-kg$ sample of water at $8\mathrm{.}5C$ is in a calorimeter. You drop a piece of steel with a mass of $0\mathrm{.}35$ kg at $209C$ into it$.$ After the sizzling subsides, what is the final equilibrium temperature? Make the reasonable assumptions that any steam produced condenses into liquid water during the process of equilibration and that the evaporation and condensation taken together don't affect the outcome, as we'll see later.

a$.$ The final equilibrium temperature of water and steel is $C.$

b$.$ If the water is in a glass beaker with a mass of $0\mathrm{.}23$ kg $,$ which in turn is in a calorimeter, with the beaker at the same temperature as the water, how will this affect the answer? Try answering before doing a detailed calculation.

Final temperature will be lower but not significantly so$.$

Final temperature will be significantly lower.

Final temperature will be significantly higher.

Final temperature will be higher but not significantly so$.$

c$.$ Using the setup in $($b$),$ the final equilibrium temperature of water, glass beaker, and steel is $\text{'}$C$.$