Calorimetry

This quiz will help you to practice calorimetry problems. In this problem, you are adding hot metal to cool water in an insulated container (i.e. your calorimeter). Remember:

q = m C ΔT

And because the heat that leaves the hot metal must enter the cool water, the common final temperature can be calculated from

-m_met C_met (T_final - T_{initial_met}) = m_water C_water (T_final - T_{initial_water})

Good luck!

Selected Specific Heats
aluminum	0.897 J g^-1 ^oC^-1
berylium	1.82 J g^-1 ^oC^-1
cadmium	0.231 J g^-1 ^oC^-1
lead	0.189 J g^-1 ^oC^-1
steel	0.466 J g^-1 ^oC^-1
uranium	0.116 J g^-1 ^oC^-1
iron	0.412 J g^-1 ^oC^-1
copper	0.386 J g^-1 ^oC^-1

Question:

31.42 g of aluminum (C = 0.897 J g^-1 ^oC^-1) initially at 97.33 ^oC is placed in 35.0 g of water (C = 4.184 J g^-1 ^oC^-1) initially at 18.69 ^oC in an insulated container. What is the final temperature when the system reaches thermal equilibrium?

Question data
metal	aluminum
Specific Heat	0.897 J g^-1 ^oC^-1
mass water	35.0 g
mass metal	31.42 g
T_i water	18.69 ^oC
T_i metal	97.33 ^oC
T_f	^oC