A 2.91 g sample of solid LiBr·H2O (s) is dissolved in 258 mL of water in a coffee cup calorimeter. Once all of the LiBr·H2O (s) is dissolved in the water, the final temperature of the solution is found to be 30.02°C. If the initial temperature of the water in the calorimeter was 20.22 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter.

The heat of solvation of LiBr·H2O (s) is -23.26 kJ/mol

Question

A 2.91 g sample of solid LiBr·H2O (s) is dissolved in 258 mL of water in a coffee cup calorimeter. Once all of the LiBr·H2O (s) is dissolved in the water, the final temperature of the solution is found to be 30.02°C. If the initial temperature of the water in the calorimeter was 20.22 °C, calculate the calorimeter constant (in J/K) for the coffee cup calorimeter. 

The heat of solvation of LiBr·H2O (s) is -23.26 kJ/mol

aaronq · Answer

use:  q=m*Cp*dT

to find q, multiply moles of LiBr*H2O by -23.26 kJ/mol

anonymous · Answer

Thanks :)