In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently us

Step 1: The given information includes the temperature change (ΔT) of the calorimeter, the heat

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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 gold weighing 19.74 grams and originally at 97.22 $^\circ$C is dropped into an insulated cup containing 85.41 grams of water at 23.99 $^\circ$C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.88 J/$^\circ$C Using the accepted value for the specific heat of gold (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings. $T_{final}$ = $^\circ$C

          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 gold weighing 19.74 grams and originally at 97.22 $^\circ$C is dropped into an insulated cup containing 85.41 grams of water at 23.99 $^\circ$C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.88 J/$^\circ$C
Using the accepted value for the specific heat of gold (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.
$T_{final}$ = $^\circ$C

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 gold weighing 19.74 grams and originally at 97.22 ^∘C is dropped into an insulated cup containing 85.41 grams of water at 23.99 ^∘C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.88 J/^∘C
Using the accepted value for the specific heat of gold (See the References tool), calculate the final temperature of the water. Assume that no heat is lost to the surroundings.
Tfinal = ^∘C

Added by Michael W.

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