An 80.0-g piece of copper, initially at 295°c, is dropped into 250 g of water contained in a 300-g aluminum calorimeter; the water and calorimeter are initially at 10.0°c.

what is the final temperature of the system? (specific heats of copper and aluminum are 0.092 0 and 0.215 cal/g⋅°c, respectively. cw = 1.00 cal/g°c)
a. 12.8°c
b. 16.5°c
c. 28.4°c
d. 32.1°c

b. 16.5°C

Explanation:

= mass of piece of copper = 80 g

= specific heat of piece of copper = 0.0920 cal/g°C

= Initial temperature of piece of copper = 295 °C

= mass of water = 250 g

= specific heat of water = 1 cal/g°C

= Initial temperature of piece of copper = 10 °C

= mass of calorimeter  = 300

= specific heat of calorimeter = 0.215 cal/g°C

= Initial temperature of calorimeter = 10 °C

= Final equilibrium temperature

Using conservation of heat

Heat lost by piece of copper = heat gained by water + heat gained by calorimeter

it may be wrong but i think its a

wavelegth as in spectrum red oygbiv