In the laboratory a \"coffee cup\" calorimeter , or constant pressure calorimete

Question

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.

A chunk of nickel weighing 18.82 grams and originally at 98.44 °C is dropped into an insulated cup containing 82.02 grams of water at 22.31 °C.

The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.82 J/°C.

Using the accepted value for the specific heat of nickel (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.

Tfinal =    °C

Explanation / Answer

mass of nickel = 18.82 g

temperature = 98.44 °C

mass of water = 82.02 grams

temperature = 22.31 °C.

The heat capacity of the calorimeter = 1.82 J/°C.

specific heat of nickel = 0.444 J / g oC

here heat loss by nickel = heat gain by water

(m Cp dT) Ni = (m Cp dT)water + Cp dT

18.82 x 0.444 x (98.44 - Tf) = 82.02 x 4.184 x (Tf - 22.31) + 1.82 x (Tf - 22.31)

8.356 x (98.44 - Tf) = 343.17 (Tf - 22.31) + 1.82 x (Tf - 22.31)

8.356 x (98.44 - Tf) = 344.992 (Tf - 22.31)

(98.44 - Tf) = 41.2867 (Tf - 22.31)

98.44 - Tf = 41.2867 Tf - 921.1

Tf = 24.11

Tfinal = 24.11 °C

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