15.0 g of ice cubes at 0.0°c are combined with 150. g of liquid water at 70.0°c in a coffee cup calorimeter. calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (the specific heat capacity of h2o(l), cs = 4.18 j/gc; h2o(s)  h2o(l) h = 6.02 kj/mol)

Answer : The final temperature will be

Explanation :

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

where,

= specific heat of ice =

= specific heat of water =

= mass of ice = 15.0 g

= mass of water = 150 g

= final temperature = ?

= initial temperature of ice =

= initial temperature of water =

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

Therefore, the final temperature will be

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.