Question

In the following experiment, a coffee-cup calorimeter containing 100 \rm mL of \rm H_2O is used. The initial temperature of the calorimeter is 23.0 \rm ^{\circ}C. If 9.80 g of \rm CaCl_2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution \Delta H_{\rm soln} of \rm CaCl_2 is \rm -82.8~kJ/mol.

Answer 1

The heat added to the calorimeter was 82,800 J x (9.80/110.98) = ?
? = mass H2O x specific heat H2O x (Tfinal-Tinitial) = 0
Substitute and solve for Tf.

Answer 2

Err.. Dr Bob do we add the mass of CaCl2 with H2O? when we want to find m