Answer:
c = 4.36 J/g°C
Step-by-step explanation:
The heat from the hot sample transfers to the cool water until equilibrium is reached.
Q-released by sample = Q-absorbed by water
Q = mcΔT
Sample:
ΔT = 99.4 - 31.8 = 67.6°C
m = 17g
c = ?
Water:
ΔT = 19.8 - 31.8 = 12°C
c = 4.18 J/g°C
Solve for c-sample:
(17g)(c)(67.6°C) = (100g)(4.18J/g°C)(12°C)
1149.2(c) = 5016
c = 4.36 J/g°C