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

the binding energy is the energy required to create z separate protons and n=a-z separate neutrons from a (a,z) nucleus in its ground state. another way to think about it is binding energy is the mass energy which is missing from a nucleus compared to the mass energy of the individual nucleons.

explanation:

newton's third law, for every action there is an equal and opposite reaction.