Answer to Question #84299 in General Chemistry for Stephanie Ezman

Question

The optimum drinking temperature for a Shiraz is 15.0 ∘C . A certain bottle of Shiraz having a heat capacity of 3.40 kJ∘C−1 is 23.1 ∘C at room temperature. The heat of fusion of ice is 6.02 kJmol−1 and the heat capacity of ice is 2.108 Jg−1∘C−1. Assume that no heat is lost to the rest of the surroundings. What minimum mass of ice, originally at -6.0 ∘C , is required to bring the final temperature to 15.0 ∘C?

Answer 1

1) Calculate how much heat you need to remove from the bottle using mc∆t ( this is a 'sensible' heat)

2) Calculate how much heat is required to take one g of ice at -6°C to water at 15°C (note there is no 'degree' with C).

This is a three part calculation:

a) sensible heat, mc∆t, to warm the ice to 0°C

b) latent heat, melting the ice

c) sensible heat, warming the water

3) Divide 1) by 2).