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"`

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 the standard Gibbs free energy change from the free energies of formation data for the following reaction: C_(6)H_(6)(l) +(15)/(2)O_(2)(g) rarr 6CO_(2)(g) +3H_(2)O(g) Given that Delta_(f)G^(Theta) =[C_(6)H_(6)(l)] = 172.8 kJ mol^(-1) Delta_(f)G^(Theta)[CO_(2)(g)] =- 394.4 kJ mol^(-1) Delta_(f)G^(Theta) [H_(2)O(g)] =- 228.6 kJ mol^(-1)

The heat of formation of NH_(3)(g) is -46 " kJ mol"^(-1) . The DeltaH (in " kJ mol"^(-1) ) of the reaction, 2NH_(3)(g)rarrN_(2)(g)+3H_(2)(g) is

Calculate the standard enthalpy of reaction ZnO(s)+CO(g)rarrZn(s)+CO_(2)(g) Given, Delta H_(f)(ZnO,s)=-350KJ//"mole",DeltaH_(f)^(@)(CO_(2),g)= -390KJ//"mole", DeltaH_(f)^(@)(CO,g)=-110KJ//"mole"

Determine enthalpy of formation for H_(2)O_(2)(l) , using the listed enthalpies of reaction : N_(2)H_(4)(l)+2H_(2)O_(2)(l)toN_(2)(g)+4H_(2)O(l) , " "Delta_(r)H_(1)^(@)=-818kJ//mol N_(2)H_(4)(l)+O_(2)(g)toN_(2)(g)+2H_(2)O(l) " "Delta_(r)H_(2)^(@)=-622kJ//mol H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l)" "Delta_(r)H_(3)^(@)=-285kJ//mol

Calculate standard free energy change from the free energy of formation data for the following reaction, C_(6)H_(6)(l)+(15)/(2)O_(2)(g)to 6CO_(2)(g)+3H_(2)O(g) . Delta_(f)G^(theta)[C_(6)H_(6)(l)]=172.8 kJ/mol Delta_(f)G^(theta)[CO_(2)(g)]=-394.4 kJ/mol Delta_(r )G^(theta)[H_(2)O(l)]=-228.6 kJ/mol

What will be the heat of reaction for the following reaction? Will the reaction be exothermic or endothermic? Fe_(2)O_(3(s))+3H_(2(g))rarr 2Fe_((s))+3H_(2)O_((l)) Delta_(f)H^(@)(H_(2)O,l)=-"285.83 kJ mol"^(-1) Delta_(f)H^(@)(Fe_(2)O_(3),s)=-"824.2 kJ mol"^(-1)

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)

Calculate the standard heat of formation of C_2H_5OH(l) from the following data: (a) C_2H_5OH (l) + 2O_2(g) to 2CO_2(g) + 3H_2O (l) , DeltaH^@ = - 1366.5 kJ (b) Delta_f H^@ [ CO_2] = -393.5 kJ mol^(-1), Delta_f H^@ [ H_2O(l)] = -285.5 kJ mol^(-1) .

Consider the reaction: 4NH_(3)(g) +5O_(2)(g) rarr 4NO(g) +6H_(2)O(l) DeltaG^(Theta) =- 1010.5 kJ Calculate Delta_(f)G^(Theta) [NO(g)] if Delta_(f)G^(Theta) (NH_(3)) = -16.6 kJ mol^(-1) and Delta_(f)G^(Theta) [H_(2)O(l)] =- 237.2 kJ mol^(-1) .