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:

A sample of aluminum (C = 0.897 J g^-1 ^oC^-1) initially at 92.57 ^oC is placed in 20.0 g of water (C = 4.184 J g^-1 ^oC^-1) initially at 23.10 ^oC in an insulated container. The final temperature is 37.66 ^oC when the system reaches thermal equilibrium. What is the mass of the metal in the sample?

Question data
metal	aluminum
Specific Heat	0.897 J g^-1 ^oC^-1
mass water	20.0 g
mass metal	g
T_i water	23.10 ^oC
T_i metal	92.57 ^oC
T_f	37.66 ^oC