Asked by mathew
A 18.3 g piece of aluminum (which has a molar heat capacity of 24.03 J/oC mol) is heated to
82.4oC and dropped into a calorimeter containing water (specific heat capacity of water is
4.18 J/goC) initially at 22.3oC. The final temperature of the water is 24.9oC. Calculate the
mass of water in the calorimeter. Ignore significant figures for this problem.
82.4oC and dropped into a calorimeter containing water (specific heat capacity of water is
4.18 J/goC) initially at 22.3oC. The final temperature of the water is 24.9oC. Calculate the
mass of water in the calorimeter. Ignore significant figures for this problem.
Answers
Answered by
DrBob222
Change 18.3 g Al to mols. mols = grams/atomic mass. Then heat lost by Al + heat gained by water = 0
[mols Al x specific heat Al x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
Solve for mass H2O after substitution.
[mols Al x specific heat Al x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
Solve for mass H2O after substitution.