Home
Class 12
CHEMISTRY
Calculate the heat of hydrogenation of C...

Calculate the heat of hydrogenation of `C_(2)H_(4)`. If `DeltaH_(f)(C_(2)H_(4))&DeltaH_(f)(C_(2)H_(6))` is `x_(1) & x_(2)` respectively:-

A

`x_(1)+x_(2)`

B

`x_(1)-x_(2)`

C

`x_(2)-x_(1)`

D

`x_(1)+x_(2)`

Text Solution

Verified by Experts

The correct Answer is:
C
`C_(2)H_(4)+H_(2) to C_(2)H_(6),DeltaH_(r)=DeltaH_(Hyd)`
`DeltaH_(r)=sumDeltaH_(f)(P)-sumDeltaH_(f)(R)`
`=x_(2)-x_(1)`.
Promotional Banner

Similar Questions

Explore conceptually related problems

When 2mole of C_(2)H_(6) are completely burnt 3129kJ of heat is liberated. Calculate the heat of formation of C_(2)H_(6).Delta_(f)H^(Theta) for CO_(2) and H_(2)O are -395 and -286kJ , respectively.

Calculate the heat of hydrogenation of C_(2)H_(2) to C_(2)H_(4) . H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l)," "DeltaH=-68.32kcal C_(2)H_(2)(g)+(5)/(2)O_(2)(g)to2CO_(2)(g)+H_(2)O(l),DeltaH=-310.61kcal C_(2)H_(4)(g)+3O_(2)(g)to2CO_(2)(g)+2H_(2)O(l),DeltaH=-337.32kcal

Calculate the heat of hydrogenation , C_(2)H_(4)(g)+H_(2)(g)toC_(2)H_(6)(g) Given that, the heats of combustion of ethylene, hydrogen and ethane are -337.0, -68.4 and -373.0 kcal respectively.

C_(2)H_(6)(g)+3.5O_(2)(g)to2CO_(2)(g)+3H_(2)O(g) DeltaS_("vap")(H_(2)O,l)=x_(1)" "cal K^(-1) (boiling point =T_(1) ) DeltaH_(f)(H_(2)O,l)" "=x_(2) DeltaH_(f)(CO_(2))" "=x_(3) DeltaH_(f)(C_(2)H_(6))" "=x_(4) Hence, DeltaH for the reaction is :

C_(2)H_(6)(g)+3.5)_(2)(g)rarr2CO_(2)(g)+3H_(2)O(g) DeltaS_(vap)(H_(2)O,l)=x_(1)calK^(-1) (boiling point =T_(1) ) DeltaH_(f)(H_(2)O,l)=x_(2) DeltaH_(f)(CO_(2))=x_(3) DeltaH_(f)(C_(2)H_(6))=x_(4) Hence, DeltaH for the reaction is

The heat of formation (DeltaH_(f)^(@)) of H_(2)O(l) is equal to :

For the equation C("diamond")+2H_(2)(g)rarrCH_(4)(g) DeltaH_(1) , C(g)+5H(g)rarrCH_(4)(g) DeltaH_(2)