Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are combined...

Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are combined with 120 g of water at 75 ∘C in an insulated container. (ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) Part A If no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using two significant figures.

Expert Solution

no of moles of ice = W/G.M.Wt = 53.5/18 = 2.97moles

heat lose of hot water = heat gain of ice

mct = ΔH∘fus*no of moles + mct

120*4.18*(75-t2) = 6020*2.97+53.5*4.18*(t2-0)

t2 = 27C⁰ >>>>>>answer

queen_honey_blossom answered 2 years ago

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Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are combined...

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