a bath contains 1000 grams of water and 100 grams of ice in thermal equilibrium. at some point in time a 500gram block of stone(granite) at 100 deg celsius is added to the bath
a) what is the temp of the bath before the block of stone is added
b) what is the temp of the bath and stone when a new equilibrium is reached?
c) how much did the entropy of the ice increase as it melted?
temp equil = (mi Ci Ti + mw Cw Tw)/((mi Ci) + (mw Cw)) where
mi = mass of ice, mw = mass of water, Ci - specific heat of ice, Cw is specific heat of water, Tw = temp of water --not given, Ti = temp of ice -- not given
i think i use a similar equation for part b, except i THINK i average the specific heats of ice and water
so for part b)
temp equil = (mb Cb Tb + ms Cs Ts)/((mb Cb) + (ms Cs)) where
mb = mass of stone, Cb = specific heat of stone, granite 1.2, Tb = temp of stone, ms = mass of ice and water, Cs = avg of specific heat of ice and water, Ts = equil temp from (a)
The Attempt at a Solution
i tried the above equations but didn't get far because the original temp of the ice and water separately was not given, the solution for part a is supposed to be 0 deg celsius but i did not get it
as for part b, i am not sure if i am even supposed to average the specific heats, when after finding out that the answer for part a was 0, i put in the Ts as 273K and used the other givens for the block and got 11.5 deg celsius -- the actual answer is supposed to be 5.13 deg celsius
i should be able to figure out part c after finding out how to get 0 for a, and 5.13 for b.
is my approach completely off? any help appreciated