Question

so I have following data but I don't know how to calculateforq

temperature of HCL 22.2 C

temperature of NaOH 21.9 C

Final temperature of resulting salt solution (Tf) 22.6 C

q=mcΔT

so m = 100 g

c=4.18 j g/C

ΔT=30.4 - ?

what is delta T? and after that how do you calculate molesofNaOH or HCL netrualized (moles of rxn)

also how do u calculate:

Enthalpy change (using expt data) for OH- + H+ --->H2O(l)

standard enthalpy of formation H2O

Calculated enthalpy of formation of OH-

please help me!!

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Hello guys. I have to do these calculations but I can seemtodo it and I am stuck. So can someone please help me calculatethesevalues?

We know that the specific heat of water (same for solutionforthis expt) is 4.18 J/g C

and densities of all solutions are 1.00 g/mL

Temp of HCl: 22.2 C

Temp of NaOH: 22.0 C

so initial Temp is average of those two which is 22.1 C

final temperature of the resulting salt solution: 22.6

so;

q=mcΔT

m= 100g

c=4.18 J/g C

ΔT= 22.6 - 22.1 = 0.5 C

so q = (100)(4.18)(0.5)

q= 209 J

so q _rxn = -q _soln

so =209 J

ok now how do you calculate moles of NaOH or HCLneutralized (molesof rxn)

once we get moles of rxn we can calculate theenthalpyof neutralization of rxn

which is calculated by q_rxn/(molesofrxn)

so how do you calculate:

enthalpy change (using expt data) for OH^-+H⁺ -> H₂O _(l)

standard enthalpy for formation H2O_(l)(ΔH)

calculated enthalpy for formation OH-_(aq)(ΔH)