4.   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

calculate the total amount of heat released = m s x Δ t
mass of the copper =m
s is the specific heat of the copper
Δ t is the change in temperature = Final (25+273)K- Initial(1358K )
after that check how much mass of water can be changed into vapors by using this heat
Heat absorbed = heat released = ms Δ t + m ΔHv for water
m is the mass of the water which is converted into steam
s is the specific heat of the copper
Δt is the change in temperature = Final (100+273)K- Initial((25+273)K )
everything is given and hence calculations are workable.