For the reaction,
`C+O_(2) rarr CO_(2),DeltaH=-393 J`
`2Zn + O_(2) rarr 2ZnO, H=-412 J`

For the reaction, C+O_(2) rarr CO_(2),DeltaH=-393 J 2Zn + O_(2) rarr 2ZnO, DeltaH=-412 J

For the reaction, C+O_(2)rarrCO_(2) , DeltaH=-393 J 2Zn+O_(2) rarr 2ZnO , DeltaH=-412J

For the reaction, C+O_(2) rarr CO_(2), DeltaH=-393J 2Zn+O_(2) rarr 2ZnO,DeltaH=-412J Which one is correct ?

For the reaction : C(s) + O_(2)(g) rarr CO_(2)(g)

In a reaction, H_(2)O +C rarr CO +H_(2)

Heat of formation of CH_(4) are: If given heat: C(s)+ O_(2)(g) rarr CO_(2) (g) " "DeltaH =-394 KJ 2H_(2) (g)+ O_(2)(g) rarr 2H_(2)O(l) rarr 2H_(2)O(l) " "DeltaH =-568 KJ CH_(4)(g) + 2O_(2)(g) rarr CO_(2)(g) + 2H_(2)O(l) " " DeltaH =- 892 KJ

Given that C + O_2 rarr CO_(2) , DeltaH^@ = -xkJ 2CO + O_2 rarr 2CO_2 , DeltaH^@ = -y kJ The enthalpy of formation of carbon monoxide will be

C_(2)H_(2) + 5/2 O_2(2) rarr 2CO_(2) + H_(2)O , Delta H = -310 kcal C + O_(2) rarr CO_(2) , " "Delta H = -94 kcal H_(2) + 1/2 O_(2) rarr H_(2)O, " " Delta H = -68 kcal On the basis of the above equations, DeltaH_(f) (enthalpy of formation) of C_2H_2 will be :