Reference no: EM13102202

At a soft drink dispenser, a restaurant patron put 0.2 kg of crushed water ice, at a temperature of ?5 C, into an insulating cup. [In fact, the ice was slightly colder before it left the machine, but its warming to ?5 C cooled the inside surface of the cup.] Then, he quickly added 0.4 kg of "pop" at a temperature of 27 C [This warm temperature arises because the refrigeration unit for the ice reservoir emits heat into its surroundings.] The speci?c heat capacity of water ice is 2100 J/(kg·C). The pop is comprised almost entirely of liquid water, and so we take its speci?c heat capacity to be [approximately] 4200 J/(kg·C). The latent heat of fusion for water is 333 kJ/kg. (a) Assuming that no heat is exchanged with the environment, determine (i) the heat required to warm the ice to 0 C, and (ii) the temperature of the pop in the cup once the ice is at 0 C. (b) Compute the amount of heat that must be absorbed by the ice to melt all of it. (c) Compute the amount of heat that would be emitted by the pop, were it to cool to 0 C. (d) Comment on your results for (b) and (c). (e) Do the problem again, this time with 0.02 kg of ice in the cup initially.