A student determines the heat of dissolution of solid potassium bromide using a coffee-cup calorimeter of negligible heat capacity When 4.49 g of KBr(s) is dissolved in 103.00 g of water, the temperature of the solution drops from 2 4.184 J/g°C 5.00 to 23.18 °C. Based on the student's observation, calculate the enthalpy of dissolution of KBr(s) in kJ/mol. Assume the specific heat of the solution is kJmol
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution(dissolving) can be determined using a coffee cup calorimeter.
In the laboratory a general chemistry student finds that when 5.07 g of CsClO4(s) are dissolved in 102.30 g of water, the temperature of the solution drops from 23.03 to 19.93 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.80 J/°C.
Based on the student's observation, calculate the enthalpy of dissolution of CsClO4(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.
ÎHdissolution = kJ/mol
b.
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution(dissolving) can be determined using a coffee cup calorimeter.
In the laboratory a general chemistry student finds that when 11.81 g of BaBr2(s) are dissolved in 118.40 g of water, the temperature of the solution increases from 22.63 to 24.39 °C.
The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.70 J/°C.
Based on the student's observation, calculate the enthalpy of dissolution of BaBr2(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat of water.