Question

A mixture containing 22.9 of ice (at exactly 0.00 ) and 76.4 of water (at 59.7 ) is placed in an insulated container. Assuming no loss of heat to the surroundings, what is the final temperature of the mixture?

45.9 ∘C

35.7 ∘C

27.5 ∘C

51.0 ∘C

Answer 1

latent heat of fusion of ice   = 334J/g-c^0
heat capacity of water         = 4.184J/g-C^0
heat capacity of ice            = 2.108J/g-C^0

Heat gain of ice   = heat lose of hot water
latent heat of ice at 0^0c to convert into water at 0^0c + heat energy of water convert to 0^0c to
final temperature t = cooling of hot water from 59.7 to final temp is t
22.9*334 + 22.9*4.184*(t-0)   = 76.4*4.184*(59.7-t)
t = 27.5^0c

27.5⁰C >>>>answer