Reference no: EM131712411

1. In Procedure II of Part 2 of the lab you will add the correct ratio of water to ice so that the final temperature of the water in the calorimeter is 0°C. Suppose you get the following data:

Mass of ice 22.9 g

Mass of water originally in the calorimeter 76.257 g

Initial temperature of water 25°C

Final temperature of water and melted ice 0°C

Determine ΔH_fusion of water given these data in KJ/Mol

2.We will use 22.5 g of ice and add it to 103.5 g of water at 25°C. Let's assume that the ice starts at 0°C (we will allow the ice to sit out for a bit of time and "dry it" so we will make this assumption). For this PreLab assignment, let's also assume we have a perfect calorimeter

So, we have"heat lost" = "heat gained"

as

Cooling the 103.5 g of water originally in the calorimeter from 25°C to the final temperature = melting the 22.5 g of ice + raising the temperature of 22.5 g of the melted ice from 0°C to the final temperature.

Given that ΔH_fusion of water = 6.0 kJ/mol, determine the theoretical final temperature of the water left in the calorimeter when the system reaches equilibrium.