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The copper(II) chloride and aluminum reaction. calculate the kilojoules of heat produced by the reaction, assuming...

The copper(II) chloride and aluminum reaction. calculate the kilojoules of heat produced by the reaction, assuming that no energy left the calorimeter.

The specific heat of the solution is 3.96J/gC ( include the mass of the aluminum foil in the total mass of the solution.

Data: Trial 1 Trial2

mass of calorimeter: 8.473g 8.610g

mass of solid Cucl2*2H2O: 3.232g 3.236g

mass of copper solution: 64.594g 62.637g

mass of aluminum foil: 0.814g 0.807g

initial temperature: 19.6C 20.8C

final temperature: 49.2C 53.4C

Solutions

Expert Solution

The specific heat of the solution is 3.96J/g^oC ( include the mass of the aluminum foil in the total mass of the solution.

Data: Trial 1

mass of calorimeter: 8.473g

mass of solid Cucl₂*2H₂O: 3.232g

mass of copper solution: 64.594g

mass of aluminum foil: 0.814g

initial temperature: 19.6^oC

final temperature: 49.2^oC

ΔT (Change in Temperature) = 49.2 -19.6 = 29.6^oC

q for trial 1 = m * C * ΔT

C = specific heat of the solution is 3.96J/g^oC

m = mass of the reactant = (mass of copper solution - mass of calorimeter - mass of solid Cucl₂*2H₂O - mass of aluminum foil) = (64.594 - 8.473 - 3.232 - 0.814 )g = 52.075 g

therefore,q for trial 1 = m * C * ΔT = 52.075g * 3.96J/g^oC *29.6^oC = 6104.02 J

1KJ = 1000J

q for trial 1 = 6.104 KJ

Data: Trial 2

mass of calorimeter: 8.610g

mass of solid Cucl₂*2H₂O: 3.236g

mass of copper solution: 62.637g

mass of aluminum foil: 0.807g

initial temperature: 20.8^oC

final temperature: 53.4^oC

ΔT (Change in Temperature) = 53.4 -20.8 = 32.6^oC

q for trial 2 = m * C * ΔT

C = specific heat of the solution is 3.96J/g^oC

m = mass of the reactant = (mass of copper solution - mass of calorimeter - mass of solid Cucl₂*2H₂O - mass of aluminum foil) = (62.637 - 8.610- 3.236 - 0.807 )g = 49.984 g

therefore,q for trial 2 = m * C * ΔT = 49.984g * 3.96J/g^oC *32.6^oC = 6452.73 J

1KJ = 1000J

q for trial 2 = 6.452 KJ

Therefore,the kilojoules of heat produced by the reaction, assuming that no energy left the calorimeter for trial 1 & trial 2 = 6.104 KJ + 6.452 KJ = 12.5567 KJ

queen_honey_blossom answered 1 year ago

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