A Piece of Iron of Mass 0 $336 ^ { \circ } \mathrm { C }$

A piece of iron of mass 0.12 kg is taken from an oven where its temperature is $336 ^ { \circ } \mathrm { C }$ and quickly placed in an insulated copper can that contains 0.20 kg of water. The copper can has mass 0.50 kg, and it and the water in it are originally at a temperature of $20 ^ { \circ } \mathrm { C }$ Calculate the final temperature of the system, assuming no heat is lost to the surroundings. Use the following specific heats: $4190 \mathrm {~J} / \mathrm { kg } \cdot \mathrm { C } ^ { \circ } \text { (water), } 470 \mathrm {~J} / \mathrm { kg } \cdot \mathrm { C } ^ { \circ } \text { (iron), }$ and $390 \mathrm {~J} / \mathrm { kg } \cdot \mathrm { C } ^ { \circ } \text { (copper). }$