An experiment was conducted in order to determine the enthalpy change that occurs when 1.0 mole of ice at 0 degrees Celsius melts and becomes 1.0 mole of water at 0 degrees Celsius. The enthalpy change associated with this process is referred to as the heat of fusion of ice. In the experiment a 9.68g sample of ice at 0 degrees Celsius was added to the coffee cup calorimeter containing 278.25 mL of distilled water. The temperature of the water was 22.485 degrees Celsius before The ice was added. The lowest temperature that was recorded after the ice had melted was 19.050 degrees Celsius. A) find the amount of heat lost or gained by the water in the calorimeter.
B) in this experiment the ice melted and then the temperature of the water produced by the ice increased from 0 degrees Celsius to 19.050 degrees Celsius. Calculate the amount of heat absorbed by the melted ice as it’s temperature increased from 0.000 degrees Celsius to 19.050 degrees Celsius
C) calculate the heat that was gained by the ice during melting process
D) calculate the heat of the fusion of ice
E) is the reaction endothermic or exothermic?
F) energy was transferred from one system to another during this experiment. Identify the two interacting systems and outline the direction of energy flow.
G) was energy conserved in the process? Justify your answer.