## Chemistry (4th Edition)

Specific heat of copper metal $s=0.139\,J/g\cdot \,^{\circ}C$ Mass $m= 366\,g$ Change in temperature $\Delta T= (12.0-77.0)^{\circ}C=-65.0^{\circ}C$ Heat transferred $q=sm\Delta T$ $=0.139\,J/g\cdot \,^{\circ}C\times366\,g\times-65.0^{\circ}C$ $=-3310\,J=-3.31\,kJ$ Negative sign indicates that the heat is liberated. 3.31 kJ heat is liberated.