Chapter 5, Problem 27E

The addition of 3.15 g of $\text{Ba}{\left(\text{OH}\right)}_2\cdot 8{\text{H}}_2\text{O}$ to a solution of 1.52 g of ${\text{NH}}_{\text{4}}\text{SCN}$ in loo g of water in a calorimeter caused the temperature to fall by 3.1 °C. Assuming the specific heat of the solution and products is 4.20 J/g °C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation:

$\text{Ba}{\left(\text{OH}\right)}_{\text{2}}\cdot {\text{8H}}_{\text{2}}\text{O}\left(s\right)+{\text{2NH}}_{\text{4}}\text{SCN}\left(aq\right)\to \text{Ba}{\left(\text{SCN}\right)}_{\text{2}}\left(aq\right)+{\text{2NH}}_{\text{3}}\left(aq\right)+\text{1}0{\text{H}}_{\text{2}}\text{O}\left(l\right)$