In an experiment to determine heat loss to a calorimeter, 100.0 mL of cool water was measured into the calorimeter and allowed to reach room temperature before 100.0 mL of heated water was added. The results of this experiment produced the data below. What is the absolute value of the calorimeter constant in J / ºC?

Question

In an experiment to determine heat loss to a calorimeter, 100.0 mL of cool water was measured into the calorimeter and allowed to reach room temperature before 100.0 mL of heated water was added.  The results of this experiment produced the data below.  What is the absolute value of the calorimeter constant in J / ºC?

ΔTheated water = -6.2 ºC
ΔTcool water= 11.2 ºC
Specific heat of water = 4.184 J deg-1 g-1
Density of water = 1 g / mL
Mass of calorimeter = 40.91 g

DrBob222 · Answer

I am confused by the wording in the problem. For example, let's say room T is 10 C so we put 100 mL of cool water in the calorimeter and the final T is 3.8 to make dT = -6.2. Then we allow the system to warm back up to 10 C? Is that right?