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Determine enthalpy of formation for H(2)...

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`

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

Calculate the standard enthaply of formation of CH_(3) OH(l) from the following data CH_(3) OH (l) + (3)/(2) O_(2) (g) to CO_(2) (g) + 2H_(2)O (l) , Delta_(r) H^(@) = - 726 kj/mol C(g) + O_(2) (g) to CO_(2) (g), Delta_(c) H^(@) = - 393 kj/mol H_(2)(g) + (1)/(2) O_(2) (g) to H_(2) O(l) : Delta_(f) H^(@) = - 286 kj /mol

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 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 enthalpy of formation of CH_(3)OH(l) from the following data: (1) CH_(3)OH(l)+(3)/(2)O_(2)(g)toCO_(2)(g)+2H_(2)O(l),Delta_(r)H^(0)=-726kJ*mol^(-1) (2) C(s)+O_(2)(g) to CO_(2)(g),Delta_(c)H^(0)=-393kJ*mol^(-1) (3) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),Delta_(f)H^(0)=-286kJ*mol^(-1) .

Substances that are oxidised and reduced in the following reaction are respectively - N_(2)H_(4)(l)+2H_(2)O_(2)(l)toN_(2)(g)+4H_(2)O(l)

Calculate the enthalpy of formation of ethyl alcohol from the following data : C_(2)H_(5)OH(l) + 3O_(2)(g) to 2CO_(2)(g) + 3H_(2)O(l), Delta_(r)H^(@) = -1368.0 kJ C(s) +O_(2)(g) to CO_(2)(g), Delta_(r)H^(@) = -393.5 kJ H_(2)(g) + 1/2O_(2)(g) to H_(2)O(l), Delta_(r)H^(@) = -286.0 kJ