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In: Chemistry

How much energy must be removed to convert 9.73 g of water at 20.9 oC to...

How much energy must be removed to convert 9.73 g of water at 20.9 oC to an ice cube at -12.0 oC? Give your answer as a positive value in Joules since only positive energy can be removed.. cwater = 4.184 J/goC, cice = 2.03 J/goC, ΔHfus, water = 6.01 kJ/mol

Solutions

Expert Solution

Ti = 20.9
Tf = -12.0
Cl = 4.184 J/g.oC
Heat released to convert liquid from 20.9 oC to 0.0 oC
Q1 = m*Cl*(Ti-Tf)
= 9.73 g * 4.184 J/g.oC *(20.9-0) oC
= 850.8457 J
Lf = 6.01KJ/mol =
6010J/mol
Lets convert mass to mol
Molar mass of H2O = 18.016 g/mol
number of mol
n= mass/molar mass
= 9.73/18.016
= 0.5401 mol
Heat released to convert liquid to solid at 0.0 oC
Q2 = n*Lf
= 0.5401 mol *6010 J/mol
= 3245.8537 J
Cs = 2.03 J/g.oC
Heat released to convert solid from 0.0 oC to -12.0 oC
Q3 = m*Cs*(Ti-Tf)
= 9.73 g * 2.03 J/g.oC *(0--12) oC
= 237.0228 J
Total heat released = Q1 + Q2 + Q3
= 850.8457 J + 3245.8537 J + 237.0228 J
= 4334 J

queen_honey_blossom answered 2 years ago
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