Ahot (70°c) lump of metal has a mass of 250 g and a specific heat of 0.25 cal/g⋅°c. john drops the metal into a 500-g calorimeter containing 75 g of water at 20°c.
the calorimeter is constructed of a material that has a specific heat of 0.10 cal/ g⋅°c.

when equilibrium is reached, what will be the final temperature? cwater = 1.00 cal/g⋅°c.

a. 114°cb. 72°cc. 64°cd. 37°c

d. 37 °C

Explanation:

= mass of lump of metal = 250 g

= specific heat of lump of metal  = 0.25 cal/g°C

= Initial temperature of lump of metal = 70 °C

= mass of water = 75 g

= specific heat of water = 1 cal/g°C

= Initial temperature of water = 20 °C

= mass of calorimeter  = 500 g

= specific heat of calorimeter = 0.10 cal/g°C

= Initial temperature of calorimeter = 20 °C

= Final equilibrium temperature

Using conservation of heat

Heat lost by lump of metal = heat gained by water + heat gained by calorimeter

no simpler subs form complex ones. synthesise = make

energy can be converted from one form to another, but it cannot be created or destroyed in ordinary chemical or physical means. do not understand what you are asking but hope this