How Does Adding Ice Affect the Final Temperature of Hot Coffee?

[salooom599]

Homework Statement

A thermos contains 160 cm^3 of coffee at 82.7 °C. To cool the coffee, you drop two 10.0-g ice cubes into the thermos. The ice cubes are initially at 0 °C and melt completely. What is the final temperature of the coffee in degrees Celsius? Treat the coffee as if it were water.

Homework Equations

Q=mL
mL=Cm(T final-T initial )

The Attempt at a Solution

i really don't know how to slove it and why there is 160 cm^3

 

[Disconnected]

Hey Salooom, Welcome to PF.
Do you have a table giving the specific latent heat (etc.) of water?
It seems that firstly you need to find the change energy required to melt the ice cubes, and the change in temperature this would cause in the coffee.
Now I'm not particularly fresh in this field, but it seems to me that you need to know the total mass of the water, do you have a value for the density of water?

Then you have some amount of water at 0*C, and some amount at a higher temperature (The original temp - the amount of heat needed to melt the cubes), and you simply work out at how much energy needs to be traded from the hot water to the cold waterfor their temperatures to be the same.

 

[salooom599]

ok i got it :D
thankss..

 

[Disconnected]

ok i got it :D
thankss..

No problem. Glad I could help (for once!)