5. In Procedure II of Part 2 of the lab you will add the correctratio of water to ice so that the final temperature of the water inthe calorimeter is 0°C. Suppose you do this and get the followingdata: Mass of ice 23.5 g Mass of water originally in thecalorimeter 73.79 g Initial temperature of water 25°C Finaltemperature of water and melted ice 0°C Determine ?Hfusion of watergiven these data. ----->5.92 kJ/mol
6. Given that ?Hfusion of water = 6.0 kJ/mol, determine thepercent error with these data
__________%
7. In Procedure I of Part 2 of the lab, you add ice to morewater than the minimum required. Questions 7-10 address thisportion of the lab. Which of the following best describes what isin the calorimeter when the system reaches equilibrium?
a. There is only water in the calorimeter and the water isgreater than 0°C.
b. There is a mixture of water and ice in the calorimeter andthe temperature of the system is less than 0°C.
c. There is a mixture of water and ice in the calorimeter andthe temperature of the system is 0°C.
d. There is a mixture of water and ice in the calorimeter andthe temperature of the system is greater than 0°C.
e. There is only water in the calorimeter and the water is0°C.
f. There is only water in the calorimeter and the water is lessthan 0°C.
8. So, you take ice out of the freezer and add it to roomtemperature water in a calorimeter (more than enough to just meltthe ice). We can determine the ?Hfusion of water by assuming we canaccount for all energy transfer and that “heat lost†is equal to“heat gainedâ€. We can assume that “heat lost†is due to which ofthe following? Check all that apply. Select all that are True.
a. Raising the temperature of ice to 0°C.
b. Cooling the calorimeter.
c. Melting the ice.
d. Raising the temperature of the melted ice from 0°C to thefinal temperature.
e. Cooling the water originally in the calorimeter.
9. We can assume that “heat gained†is due to which of thefollowing? Check all that apply. Select all that are True.
a. Melting the ice.
b. Raising the temperature of the melted ice from 0°C to thefinal temperature.
c. Cooling the calorimeter.
d. Raising the temperature of ice to 0°C.
e. Cooling the water originally in the calorimeter.
10. We will use 29.1 g of ice and add it to 128.04 g of water at25°C. Let’s assume that the ice starts at 0°C (we will allow theice to sit out for a bit of time and “dry it†so we will make thisassumption). For this PreLab assignment, let’s also assume we havea perfect calorimeter (you will judge this assumption in Part 1 ofthe lab). So, we have “heat lost†= “heat gained†as Cooling the128.04 g of water originally in the calorimeter from 25°C to thefinal temperature = melting the 29.1 g of ice + raising thetemperature of 29.1 g of the melted ice from 0°C to the finaltemperature. Given that ?Hfusion of water = 6.0 kJ/mol, determinethe theoretical final temperature of the water left in thecalorimeter when the system reaches equilibrium._____ °C
