A $25\mathrm{.}4$g piece of iron and a $24\mathrm{.}2$g piece of gold at $100\mathrm{.}0$ degrees celsius were dropped into $610\mathrm{.}0$mL of water at $27\mathrm{.}0$ degrees Celsius. The molar heat capacities of iron and gold are $25\mathrm{.}19$J$/$mol$*$degree celsius and $25\mathrm{.}41$J$/$mol$*$degree celsius, respectively. What is the final temperature of the water and pieces of metal?

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This is a calorimetry problem where we apply the conservation of energy which essentially states tha... View the full answer