A calorimeter contains 100 g of water at 25°C. You heat a 100 g copper block to its melting point (1,358 K) and plunge it in the calorimeter. Assume that the final temperature of the block reaches 25°C. How much heat was released from the copper block? At the end of the experiment, how many grams of water are liquid and at what temperature? How many grams of water are steam and at what temperature? Show your work.
Specific heat of liquid water = 4.18 J/g–°C
Specific heat of copper = 0.385 J/g–°C
ΔHv for water = 40.7 kJ/mol
Amount of heat released
q = m s delta t
m=100g
s= 0.385 J/g–°C
delta t = 298- 1358
q= 40810J
The calculations can be done to calculate the amount of heat released by copper block
This is the amount of heat gained by 100 g of water
Now heat required to raise the temp of water to 100 degree C =m s delta t = 100 x 4.18 x ( 75) J =31350J
heat required to convert 100g (100/18 moles) of water into steam at 100 degree C = m delta Hv = 5.55 x 40.7 = 226100J
Total heat required = 31350+226100J
Total heat available is 40810J