For a cell,
`4B(s)+3O_(2)(g)rarr2B_(2)O_(3)(g)`; `E_(cell)^(0)=1.433` volt
What is molar entropy (in `J/K`) of oxygen gas
Given:`(Delta_(f)H^(0))_(B_(2)O_(3))(g)=-840(kJ)/(mol)`
`(S_(m)^(0))_(B_(2)O_(3))(g)=280J/(K-mol)`
`(S_(m)^(0))_(B)(s)=10J/(K-mol)`

What is the normal boiling point of mercury? Given : DeltaH _(f)^(@)(Hg,l)=0,S^(@)(Hg,l)=77.4 J//K-"mol" DeltaH _(f)^(@)(Hg,g)= 60.8 kJ//"mol", S^(@)(Hg, g)=174.4 J//K-"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"

Diborane is a potentail rocket fuel which undergoes combusion according to the reaction B_(2)H_(6)(g)+3O_(2)(g)rarrB_(2)O_(3)(s)+3H_(2)O(g) From the following data, calculate the enthalpy change for the combustion of diborane 2B(s)+(3//2)O_(2)(g)rarrB_(2)O_(3)(s) DeltaH= -1273 kJ mol^(-1) H_(2)(g)+(1//2)O_(2)(g)rarrH_(2)O(1) " "Delta H= -286 kJ mol^(-1) H_(2)O(1)rarrH_(2)O(g)" "DeltaH=44 kJ mol^(-1) 2B(s)+3H_(2)(g)rarrB_(2)H_(6)(g)" "Delta H= 36kJ mol^(-1)

Calculate standard entropy change in the reaction Fe_(2)O_(3)(s)+3H_(2)(g) rarr 2Fe(s)+3H_(2)O(l) Given : S_(m_(0))(Fe_(2)O_(3).S)=87.4,S_(m)^(@)(Fe,S)=27.3 S_(m)^(@)(H_(2),g)=130.7,S_(m)^(@)(H_(2)O,l)=69.9JK^(-1)mol^(-1)

Calculate the change in entropy for the following reaction 2CO(g) +O_(2)(g) rarr 2CO_(2)(g) Given: S_(CO)^(Theta)(g)=197.6 J K^(-1)mol^(-1) S_(O_(2))^(Theta)(g)=205.03 J K^(-1)mol^(-1) S_(CO_(2))^(Theta)(g)=213.6 J K^(-1)mol^(-1)

For the reaction: CO(g) +H_(2)O(g) hArr CO_(2)(g) +H_(2)(g) (Delta_(r)H)_(300K) = - 41.2 kJ mol^(-1) (Delta_(r)H)_(1200K) =- 33.0 kJ mol^(-1) (Delta_(r)S)_(300K) = - 4.2 xx 10^(-2) kJ mol^(-1) (Delta_(r)S)_(1200K) =- 3.0 xx10^(-2) kJ mol^(-1) Predict the direction of spontaneity of the reaction at 300K and 1200K . also calculated log_(10)K_(p) at 300K and 1200K .

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"

Find out InK_(eq) for the formation of NO_(2) from NO and O_(2) at 298 K NO_(g)+(1)/(2)O_(2)hArrNO_(2)g Given: DeltaG_(f)^(@)(NO_(2))=52.0KJ//mol e Delta_(f)^(@)(NO)=87.0KJ//mol e Delta_(f)^(@)(O_(2))=0KJ//mol e

Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )G^(@) at 320 K is :

Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: CH_(3)OH(l)+3/2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l), …(i), Delta_(r)H_(1)^(Θ)=-726 kJ mol^(-1) C(g)+O_(2)(g) rarr CO_(2)(g), …(ii), Delta_(c )H_(2)^(Θ)=-393 kJ mol^(-1) H_(2)(g)+1/2O_(2)(g) rarr H_(2)O(l), ...(iii), Delta_(f)H_(3)^(Θ)=-286 kJ mol^(-1)