Acoffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. a 10.0 g sample of an ionic compound with a molar mass of 145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. after stirring and dissolving the solid, the temperature was found to change from 25.00 ∘c to 23.89 ∘c . calculate the enthalpy of solution, δhsoln , per mole of salt dissolved. assume the specific heat of the solution is 4.06 j/(g⋅∘c ) and the heat capacity of the calorimeter is 5.10 j/ ∘c . calculate the heat change experienced by the calorimeter contents, . = j calculate the heat change experienced by the calorimeter, . = j calculate the heat change produced by the solution process, . = j calculate δhsoln , the enthalpy of solution for one mole of solid in kilojoules per mole. δhsoln= kj/mol

The enthalpy of solution for one mole of solid is 4.003 kilojoules per mole.

Explanation:

Heat lost by the resultant solution that is content of calorimeter=

= change in temperature =  -1.11°C

Heat lost by the calorimeter =

= change in temperature =  -1.11°C

Heat absorbed by the reaction = Heat lost by solution + Heat lost by the calorimeter

where,

Q = heat absorbed by the reaction or heat change due to solution process

= specific heat of solution =

= specific heat of calorimeter=

= mass of solution= 60.0 g

= change in temperature =  -1.11°C

Now put all the given values in the above formula, we get:

Heat change due to solution process is 276.057 J.

Now we have to calculate the enthalpy change for dissolving this salt on a energy per mole

where,

= enthalpy change = ?

q = heat absorbed = 276.057 J

m = mass of salt = 10.0  g

n = mole of salt =

The enthalpy of solution for one mole of solid is 4.003 kilojoules per mole.