Intial volume of water in the styrofoam cup (before the ice was added) (mL)
Final volume of water in the styrofoam cup (after the ice melted) (mL)
Volume of water due to melted ice (mL)
Mass (g) melted ice
Initial temperature (°C) of the water placed in the styrofoam cup
Minimum temperature (°C) after the ice was melted
1. The amount of liquid water placed in the cup was _____100_______ mL. Assume that the density of water is 1.0 g/mL. What is the weight in grams of the liquid water?
Yes, because the density of water is 1
2. Calculate the temperature change.
3. Knowing that the specific heat of water is 4.184 J/g°C, calculate the total amount of heat released by the 100 ml of water as it cooled. This energy was used to melt the ice and then raise the temperature of the melted ice from 0 °C to the minimum temperature of the system. …show more content…
The amount of heat lost by the liquid water was _______18200.4j_______. Assuming that the Law of Conservation of Energy applies, the amount of heat absorbed by the melting ice was ___________8660.52___.
5. Calculate the volume of water contributed to the cup by the melted ice.