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

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 silver weighing 18.10 grams and originally at 98.24 °C is dropped into an insulated cup containinghemomneter 79.03 grams of water at 23.40 °C Stirring rod The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.63 Joc. Water Metal sample Using the accepted value for the specific heat of silver (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings. final

Explanation / Answer

Q1

Qsilver= m*C*(Tf-Ti) = 18.1*0.23*(Tf-98.24)

Qwater = m*C*(Tf-Ti) = 79.03*4.84*(Tf-23.40)

Qcal = Ccal*(Tf-Ti) = 1.63*(Tf-23.40)

and we know

-Qsilver = Qwater + Qcal

-18.1*0.23*(Tf-98.24) = (79.03*4.84+1.63)*(Tf-23.40)

-4.163Tf + 98.24*4.163 = 384.1352Tf -23.40*384.1352

Tf(-4.163 - 384.1352) = -23.40*384.1352-98.24*4.163

Tf = -9397.7368 / -388.29

Tf = 24.2°C

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