Four ice cubes at exactly 0 ?C with a total mass of 52.5g are combined with...

Four ice cubes at exactly 0 ?C with a total mass of 52.5g are combined with 145g of water at 75?C in an insulated container. (?H?fus=6.02 kJ/mol, cwater=4.18J/g??C)

If no heat is lost to the surroundings, what is the final temperature of the mixture?

T=?

Expert Solution

heat released = heat absorbed

Let T2 be the final temperature

heat released by the water = m * Cp * (T2-T1)

= 145g * 4.18J/g^oC * (T2-75)

heat absorbed by the water = m * Cp * (T2-T1) + Hfus * number of moles of ice

number of moles of ice = 145/18 = 8.06 moles

heat absorbed by the water = m * Cp * (T2-T1) + Hfus * number of moles of ice

= 52.5g * 4.18J/g^oC * (T2-0) + 6.02 kJmol^-1*8.06

= 219.45 (T2-0) + 48.52

-[219.45 (T2-0) + 48.52] = 145g * 4.18J/g^oC * (T2-75)

T2 = 55 ^oC

final temperature is 55 ^oC

queen_honey_blossom answered 4 months ago

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Four ice cubes at exactly 0 ?C with a total mass of 52.5g are combined with...

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