This problem is providing us with the initial temperature of 40 g of ice as -15 °C, so the heat involved in the process to heat it up to 16.5 °C is required as well as the type of process, endothermic or exothermic. At the end, we obtain 17.4 kJ as the total heat and the process to be endothermic.
Energy in phase changes:
In chemistry, we can quantify the energy that is involved in a phase change by considering every sub-process that takes place from the initial temperature to the final one. In such a way, since this block of ice must first heat to 0 °C, then melt and finally heat to 16.5 °C, one infers three heat terms are needed; two sensible-based and one latent-based:
[tex]Q_T=Q_1+Q_2+Q_3[/tex]
Hence, we define and calculate each term as follows:
[tex]Q_1=m*C_{ice}*(0\°C-(-15\°C))=40g*2.093\frac{J}{g*\°C}(15\°C)=1255.8J\\ \\Q_2=m*\Delta _mH=40g*333.55\frac{J}{g} =13342J\\\\Q_3=mC_{water}(16.5\°C-0\°C)=40g*4.184\frac{J}{g*\°C}(16.5\°C)=2761.4J[/tex]
Finally, we add them together to obtain:
[tex]Q_T=17359.2J*\frac{1kJ}{1000J}\\ \\Q_T=17.4kJ[/tex]
Learn more about enthalpy of melting: brainly.com/question/4335686
