Question

Suppose two 45-g ice cubes are added to a glass containing 500 cm3 of cola at 20,0°C.
When thermal equilibrium is reached, all the ice will have melted, and the temperature of
the mixture will be somewhere between 20,0°C and 0°C. Calculate the final temperature
of the mixture. You may assume that the cola has a density and specific heat capacity the
same as water namely:
Density = 1,0 g/cm3 and specific heat = 4,184 J/gK
The heat of fusion (of water) is 333J/g.

Answer 1

how much heat from the cola to melt the ice?

then just equalize the water temperature

Answer 2

5. Suppose four 30-g ice cubes are added to a glass containing 200 cm3 of orange juice at
20,0°C.
You may assume that the orange juice has a density and specific heat capacity the same
as water namely: Density = 1,0 g∙cm–3 and specific heat = 4,184 J/gK
The heat of fusion (of water) is 333 J/g.
Your task is twofold. You must determine:
a) Whether or not all the ice will melt; and
b) If your finding is that some ice will be left in the juice, you must calculate what mass
of ice will be present the moment when thermal equilibrium is reached

Answer 3

How much heat is needed to melt 120 g ice? That's 120 g x 333 = 39960 J.
How much heat can be obtained from the OJ going from 20 to 0 C? That's
200 x 4.184 x 20 = 16,376 J
So you don't have enough heat in the O.J. to melt all of the ice. How much ice can melt with 16,376 J. Subtract from 120 g to see how much is left.

Answer 4

0,49