What is the enthalpy of neutralization of HF against a strong base?
Given : `H^(+)(aq)+OH^(-)(aq)rarrH_(2)O(l),Delta_(r)H^(@)=-56kJ//mol`
`Delta_(s)H^(@)(HF,aq)=-329kJ//mol,Delta_(s)H^(@)(H_(2)O,l)=-285kJ//mol`
`Delta_(s)H^(@)(F^(-),aq)=-320 " kJ"//"mol"`

The fat, C_(57)H_(104)O_(6)(s) , is metabolized via the following reaction. Given the enthalpies of formation, calculate the energy (kJ) liberated when 1.0 g of this fat reacts. C_(57)H_(104)O_(6)(s)+80 O_(2)(g)rarr57CO_(2)(g)=-52 H_(2)O(l) Delta_(f)H^(@)(C_(57)H_(104)O_(6),s)=-70870" kJ"//"mol, "Delta_(f)H^(@)(H_(2)O,l)=-285.8 " kJ"//"mol" , Delta_(f)H^(@)(CO_(2),g)=-393.5 " kJ"//"mol"

The fat, C_(57)H_(104)O_(6)(s) , is metabolized via the following reaction. Given the enthalpies of formation, calculate the energy (kJ) liberated when 1.0 g of this fat reacts. C_(57)H_(104)O_(6)(s)+80 O_(2)(g)rarr57CO_(2)(g)+52 H_(2)O(l) Delta_(f)H^(@)(C_(57)H_(104)O_(6),s)=-70870" kJ"//"mol, "Delta_(f)H^(@)(H_(2)O,l)=-285.8 " kJ"//"mol" , Delta_(f)H^(@)(CO_(2),g)=-393.5 " kJ"//"mol"

Calculate enthalpy of ionisation of OH^(-) ion. Given: H_(2)O_((l)) to H_((aq))^(+) + OH_((aq))^(-) , DeltaH^(@) = -285.83 KJ

Determine the enthalpy of formation of B_(2)H_(6) (g) in kJ/mol of the following reaction : B_(2)H_(6)(g)+3O_(2)(g)rarrB_(2)O_(3)(s)+3H_(2)O(g) , Given : Delta_(r )H^(@)=-1941 " kJ"//"mol", " "DeltaH_(f)^(@)(B_(2)O_(3),s)=-1273" kJ"//"mol," DeltaH_(f)^(@)(H_(2)O,g)=-241.8 " kJ"//"mol"

Determine the enthalpy of formation of B_(2)H_(6) (g) in kJ/mol of the following reaction : B_(2)H_(6)(g)+3O_(2)(g)rarrB_(2)O_(3)(s)+3H_(2)O(g) , Given : Delta_(r )H^(@)=-1941 " kJ"//"mol", " "DeltaH_(f)^(@)(B_(2)O_(3),s)=-1273" kJ"//"mol," DeltaH_(f)^(@)(H_(2)O,g)=-241.8 " kJ"//"mol"

Determine the enthalpy of formation of B_(2)H_(6) (g) in kJ/mol of the following reaction : B_(2)H_(6)(g)+3O_(2)(g)rarrB_(2)O_(3)(s)+3H_(2)O(g) , Given : Delta_(r )H^(@)=-1941 " kJ"//"mol", " "DeltaH_(f)^(@)(B_(2)O_(3),s)=-1273" kJ"//"mol," DeltaH_(f)^(@)(H_(2)O,g)=-241.8 " kJ"//"mol"

From the following data, mark the option (s) where Delta H is correctlt written for the given reaction. Given H^(+)(aq) + OH^(-)(aq) rarr H_(2)O(l), Delta H = -57.3 kJ Delta H_("solution") of HA(g) = -70.7kJ/mol Delta H_("solution") of BOH(g) = 20kJ/mol Delta H_("ionization") of HA = 15 kJ/mol and BOH is a strong base Reaction Delta H_(r)(kJ//mol)

Determine C-C and C-H bond enthalpy (in kJ//mol ) Given : Delta_(f)H^(@)(C_(2)H_(6),g)=-85kJ//mol," "Delta_(f)H^(@)(C_(3)H_(8),g)=-104kJ//mol Delta_("sub")H^(@)(C,s)=718kJ//mol," "B.E.(H-H)=436kJ//mol

Determine C-C and C-H bond enthalpy (in kJ//mol ) Given : Delta_(f)H^(@)(C_(2)H_(6),g)=-85kJ//mol," "Delta_(f)H^(@)(C_(3)H_(8),g)=-104kJ//mol Delta_("sub")H^(@)(C,s)=718kJ//mol," "B.E.(H-H)=436kJ//mol