An 920-G Piece of Iron At $100 ^ { \circ } \mathrm { C }$

An 920-g piece of iron at $100 ^ { \circ } \mathrm { C }$ is dropped into a calorimeter of negligible heat capacity containing 50 g of ice at $0 ^ { \circ } \mathrm { C }$ and 92 g of water, also at $0 ^ { \circ } \mathrm { C }$ What is the final temperature of the system? The specific heat of iron is 448 $\mathrm { J } / \mathrm { kg } \cdot \mathrm { K }$ that of water is 4186 $\mathrm { J } / \mathrm { kg } \cdot \mathrm { K } _ { 1 }$ , and the latent heat of fusion of water is $33.5 \times 10 ^ { 4 } \mathrm {~J} / \mathrm { kg }$

A) $32 ^ { \circ } \mathrm { C }$
B) $0 ^ { \circ } \mathrm { C }$
C) $11 ^ { \circ } \mathrm { C }$
D) $24 ^ { \circ } \mathrm { C }$
E) $14 ^ { \circ } \mathrm { C }$