A 360-g metal container, insulated on the outside, holds 180.0 g of water in thermal equilibrium at $22.0 ^ { \circ } \mathrm { C }$ A 24.0-g ice cube, at the melting point, is dropped into the water, and when thermal equilibrium is reached the temperature is $15.0 ^ { \circ } \mathrm { C }$ Assume there is no heat exchange with the surroundings. For water, the specific heat capacity is $4190 \mathrm {~J} / \mathrm { kg } \cdot \mathrm { K }$ and the heat of fusion is $3.34 \times$ $10 ^ { 5 } \mathrm {~J} / \mathrm { kg }$ What is the specific heat capacity of the metal of the container?

Question

A 360-g metal container, insulated on the outside, holds  180.0 g of water in thermal equilibrium at $22.0 ^ { \circ } \mathrm { C }$ A  24.0-g ice cube, at the melting point, is dropped into the water, and when thermal equilibrium is reached the temperature is $15.0 ^ { \circ } \mathrm { C }$ Assume there is no heat exchange with the surroundings. For water, the specific heat capacity is $4190 \mathrm {~J} / \mathrm { kg } \cdot \mathrm { K }$ and the heat of fusion is $3.34 \times$ $10 ^ { 5 } \mathrm {~J} / \mathrm { kg }$ What is the specific heat capacity of the metal of the container?

Quizplus · Accepted Answer

The Answer of A 360-g metal container, insulated on the outside, holds  180.0 g of water in thermal equilibrium at $22.0 ^ { \circ } \mathrm { C }$ A  24.0-g ice cube, at the melting point, is dropped into the water, and when thermal equilibrium is reached the temperature is $15.0 ^ { \circ } \mathrm { C }$ Assume there is no heat exchange with the surroundings. For water, the specific heat capacity is $4190 \mathrm {~J} / \mathrm { kg } \cdot \mathrm { K }$ and the heat of fusion is $3.34 \times$ $10 ^ { 5 } \mathrm {~J} / \mathrm { kg }$ What is the specific heat capacity of the metal of the container?

A 360-G Metal Container, Insulated on the Outside, Holds 22.0∘C22.0 ^ { \circ } \mathrm { C }22.0∘C

A 360-G Metal Container, Insulated on the Outside, Holds $22.0 ^ { \circ } \mathrm { C }$