Specific heat capacity questions:

A metal ring with a mass of 21.61 g undergoes a change in temperature of 32.67 oC. The energy change, or heat, required for this change in temperature is 1563 Joules.
What is the specific heat of the ring?

P.1.13 A 8.0 kg piece of zinc at 75 degrees Celsius is placed in a container of water. The water has a mass of 20 kg and has a temperature of 11.0 degrees Celsius before the zinc is added. What is the final temperature of the water and zinc?

heat capacity is a property that looks how adding/subtracting heat to/from a material increases/decreases the temperature of that material.

heat capacity = C = heat transferred / change in temperature = C = q / ∆T
specific heat capacity = heat transferred / ( change in temperature x mass of material) = Cs = q / (m∆T) = ∆H / (m∆T)

Cs of the metal ring = ∆H / (m∆T) = 1563 J / (21.61 g x 32.67oC) = 2.214 J/g-oC
or, using the kelvin temperature scale = 1563 J / [21.61 g x (32.67 + 273.15) K] = 0.2365 J/g-K



use the fact that heat lost by the zinc = heat gained by the water

Cs = q / (m∆T)
q = Cs(m∆T).
q(zinc) = Cs(zinc) *m(zinc) *∆T
q(water) = Cs(water) *m(water)*∆T
and q(zinc) = q(water)

so Cs(zinc) *m(zinc) *∆T(zinc) = Cs(water) *m(water)*∆T(water)

use Cs (zinc) = 0.3895 J/(g•K) , Cs(water) = 4.184 J/(g•K) at about room temperature
convert the temperatures from celsius scale to kelvin scale (add 273)

(0.3895 J/(g•K) ) (8000 g zinc) (348 K - final temperature) = (4.184 J/(g•K)) (20,000) (final temperature - 284 K)

(348 K - final temperature) / (final temperature -284 K) = 26.85 J/K

final temperature = 286.3 K = 13.3 oC

1563 J = (21.61 g) (32.67 ℃) (x)

x = 2.214 J/g ℃

For your second problem, go here:

http://www.chemteam.info/Thermochem/Mixi…

You'll need the specific heat of zinc and water. Water is 4.184 J/g ℃ and zinc is 0.39 J/g ℃.