A45.9 g sample of a metal is heated to 95.2°c and then placed in a calorimeter containing 120.0 g of water (c = 4.18 j/g°c) at 21.6°c. the final temperature of the water is 24.5°c. which metal was used?

Iron

Explanation:

Heat released by the metal sample will be equivalent to the heat absorbed by  water.

But heat = mass × specific heat capacity × temperature change

Thus;

Heat released by the metal;

= 45.9 g × c ×(95.2 -24.5) , where c is the specific heat capacity of the metal

= 3245.13c joules

Heat absorbed by water;

= 120 g × 4.18 J/g°C × (24.5-21.6)

= 1454.64 joules

Therefore;

3245.13c joules = 1454.64 joules

c = 1454.64/3245.13

  = 0.448 J/g°C

The specific heat capacity of the  metal sample is 0.448 J/g°C. The metal use is most likely, Iron.

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

it takes on an electronical energy