A 11.6 g piece of metal is heated to 98°C and dropped into a calorimeter containing 50.0 g of water (specific heat capacity of water is 4.18 J/g°C) initially at 20.5°C. The empty calorimeter has a heat capacity of 125 J/K. The final temperature of the water is 28.2°C. Ignoring significant figures, calculate the specific heat of the metal.

Answer : The specific heat of the metal is,

Explanation :

Heat released by the reaction = Heat absorbed by the calorimeter + Heat absorbed by the water

where,

q = heat released by the reaction

= heat absorbed by the calorimeter

= heat absorbed by the water

c = specific heat of metal = ?

= specific heat of calorimeter =

= specific heat of water =

= mass of water = 50.0 g

m = mass of metal = 11.6 g

= final temperature =

= temperature of metal =

= temperature of water =

Now put all the given values in the above formula, we get:

Thus, the specific heat of the metal is,

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.