- #1
jackal22
- 2
- 0
ok i keep reading that ideally they (neutralisation enthalpies) are meant to be around 58KJ
here is my problem:
im reacting 50cm3 of NaOH with 25cm3 of HCl
the HCl is 1 mole NaOH is also 1 mole.
my moles calculation is: (1x25)/1000 which gives me 0.025
the i do :
((mass x specific heat x change in temp)/moles)/1000
i get -25.4 which is no where near 58 ish...
same thing when i use nitric acid instead, i end up with 27.08. However when i use sulphuric acid i get a result of 52.416 (sulphuric acid is 0.5 molar)
so my question is, am i getting something wrong? I am using the mass of the substance needed to neutralise the acid for mass (reading it off a graph) & I am using 4.2 for specific heat
also is there any reason for why some are better at neutralising is it like to do with more H+ ions ?
i would really appreciate any help
here is my problem:
im reacting 50cm3 of NaOH with 25cm3 of HCl
the HCl is 1 mole NaOH is also 1 mole.
my moles calculation is: (1x25)/1000 which gives me 0.025
the i do :
((mass x specific heat x change in temp)/moles)/1000
i get -25.4 which is no where near 58 ish...
same thing when i use nitric acid instead, i end up with 27.08. However when i use sulphuric acid i get a result of 52.416 (sulphuric acid is 0.5 molar)
so my question is, am i getting something wrong? I am using the mass of the substance needed to neutralise the acid for mass (reading it off a graph) & I am using 4.2 for specific heat
also is there any reason for why some are better at neutralising is it like to do with more H+ ions ?
i would really appreciate any help