Calculate the enthalphy change for the process H2SO4(l) -> H2SO4(aq), in kJ.mol.?

Question

You should use care when dissolving H2SO4 in water because the process is highly exothermic. To measure the enthalphy change, 5.2g H2SO4 (l) was added (with stirring) to 135g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 20.2 degrees C to 28.8 C.

Calculate the enthalphy change for the process
H2SO4(l) -> H2SO4(aq), in kJ.mol.

Answer 1

Molecular mass of H2SO4: 98.07848 g/mol
After 5.2g H2SO4 (l) was added (with stirring) to 135g of water, the total mass is: 140.2g. Assume that heat capacity of this solution is still the same as that of water: 4.182 J/g.C. So the total heat released is:
140.2*4.182*8.6 = 5.042 kJ
5.2g H2SO4 is 5.2/98.07848 = 0.053 Mole.
So the enthalpy change for the process is:
5.042 kJ/0.053 Mole = 95.1 kJ/mol

Answer 2

in the given equation H denotes enthalpy and deltaH is the enthalpy replace. word that the reaction is balanced. as a result, for 2 moles of CO fed on, the enthalpy replace (i.e., deltaH) is 22.2 kj. => for a million mole of CO fed on, deltaH = 22..2kj/2 = 11.a million kj => for 5 moles of CO fed on, deltaH = 11.a million kj *5 = fifty 5.5kj.