Answer:
5.61°C
Explanation:
The heat transferred (Q) is equal to the mass (m) times the specific heat capacity (C) times the change in temperature (ΔT). For a phase change, such as melting solid ice to liquid water at 0°C, the heat transferred is equal to the mass times the latent heat (L).
The heat gained by the ice = the heat lost by the water
The ice is heated to 0°C, then melted, then warmed as liquid water to the final equilibrium temperature.
[tex]\large \text {$ Q_{ice}+Q_{melt}+Q_{liquid}=-Q_{water} $}\\\large \text {$ m_{ice}C_{ice}(0-T_{ice})+m_{ice}L_{fusion}+m_{ice}C_{water}(T-0)=-m_{water}C_{water}(T-T_{water}) $}[/tex]
Plugging in values:
[tex]\text {$ (0.35)(2030)(0-(-15))+(0.35)(3.35\times10^5)+(0.35)(4180)(T-0)=-(0.61)(4180)(T-59) $}\\\large \text {$ 10,657.5+117,250+1463\ T=-2549.8\ T+150,438.2 $}\\\large \text {$ 4012.8\ T=22,530.7 $}\\\large \text {$ T=5.61 $}[/tex]
