40.0 g of ice cubes at 0.0 $\degree$C are combined with 150. g of liquid water at 20.0 $\degree$C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H₂O(l), c = 4.18 J/g- $\degree$C; H₂O(s) $\rightarrow$ H₂O(l) $\Delta$H = 6.02 kJ/mol)

Question

Quizplus · Accepted Answer

The ice will melt and absorb heat from the water until thermal equilibrium is reached. The heat required to melt the ice is less than the heat the water can provide, so the final temperature will be 0.0°C.

400 G of Ice Cubes at 0 °\degree° C Are Combined with 150

400 G of Ice Cubes at 0 $\degree$ C Are Combined with 150