Chemistry HW HELP!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!! (This is really an emergency!!!)?

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

This is a pretty straightforward problem which you would have gotten a faster answer to if you put it in the chemistry section, eh?

OK, the coffee is going to cool down from the ice. How much will it cool down?

First you have to warm up the ice to 0 degrees so that it can start to melt. So figure how many calories it takes to warm 23 g of ice by 2.2 degrees.

OK, now you have to melt 23 g of ice. So figure out how many calories it takes to do that.

Those calories have to be removed from the temperature of the coffee. So you have to reduce the temp of the coffee enough to give you those calories. One degree drop of temp of the coffee gives you a callorie for each mL of coffee, right?

OK, so now you have 23 g of water at 0 degrees, and 248 mL of coffee at a little less than 98 degrees. It's a little equation - the temp of the 23 g plus the temp of the 248 mL will give the temp of the total of 271 g (or ML)

Piece of cake.