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.

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons