HELP!!!!!!! Chemistry HW HELP!!!!!!!?

Question

At a local convenience store, you purchased a cup of coffee but, at 98.4 Degrees Celcius, it is too hot to drink. You add 23.0g of ice that is -2.2 Degrees Celsius to 248 mL of the coffee. What is the final temperature of the coffee? (assume the heat capasity and density of the coffee are the same as water and the coffee cup is well insulated.)

Answer 1

let thetemperature of the mix be 't'*Cfind the heat lost by coffee
find the heat gained by ice in three stages
a)from -2.2*C to 0*C
b)for melting and becoming water at 0*C
c)for getting to the equilibrium temperature of the mixture
equate and solve

Answer 2

Cute example that does not work in real life.

Adding the ice changes the chemical composition of the coffee rendering all standard heat exchange formulas useless. When this is done, the cooling effect of the ice might cool it, but it may also increase the temerature of the system as well.

The better way to cool off coffee is by inserting a dairy based liquid into the equation, such as milk or creamers. These have a super cooling effect on the coffee, cooling it down more than the general heat exchange formulas suggest it would.

Answer 3

i think you just do:
Q(ice) = mass*specific heat of ice*change in Temperature
Q(coffee) = mass*specific heat of coffee* change in Temperature
then do Q(ice) + Q(coffee) and that gives you an equation where you can solve for final Temperature.

and since heat capacity and density are the same as water, i think the specific heat of coffee will just equal 1.

* = multiply

Answer 4

This is Physics, not Chemistry.

Heat Gain by Ice = Heat loss by coffee

Constants like specific heat capacity of ice, specific latent heat of fusion of water needs to be provided. I don't specific heat capacity of ice is also 4200J/KgK.