Home
Class 12
CHEMISTRY
The heat of formation of NH(3)(g) is -46...

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

A

46

B

`-46`

C

92

D

`-92`

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Similar Questions

Explore conceptually related problems

The enthalpy of formation of ammonia is -46.0 KJ mol^(-1) . The enthalpy change for the reaction 2NH_(3)(g)rarr N_(2)(g)+3H_(2)(g) is :

The value of Delta_(f) H^(Θ) for NH_(3) is -91.8 kJ mol^(-1) . Calculate enthalpy change for the following reaction. 2NH_(3) (g) rarr N_(2) (g) + 3H_(2) (g)

For the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g), DeltaH=?

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"

Silanes are silicon hydrides of general formula Si_(n)Hn_(2n+2) and have several applications. From the data given below, the bond dissociation enthalpy of Si-Si bond ("in kJ mol"^(-1)) is Given: DeltaH of the reaction 2Si(s)+3H_(2)(g)rarrSi_(2)H_(6)(g)" is "80.3 kJ mol"^(-1) Bond dissociation enthalpy for H-H=436" kJ mol"^(-1) Bond dissociation enthalpy for Si-H=304" kJ mol"^(-1) Delta_(f)H[Si(g)]="450 kJ mol"^(-1)

Bond dissociation enthalpies of H_(2(g)) and N_(2(g)) are "426.0 kJ mol"^(-1) and "941.8 kJ mol"^(-1) , respectively, and enthalpy of formation of NH_(3(g))" is "-"46 kJ mol"^(-1) . What are the enthalpy of atomisation of NH_(3(g)) and the average bond enthalpy of N-H bond respectively ( in kJ "mol"^(-1) )?

Bond dissociation enthalpies of H_(2)(g) and N_(2)(g) are 436.0 kJ mol^(-1) and 941.8 kJ mol^(-1) , respectively, and ethalpy of formation of NH_(3)(g) is -46kJ mol^(-1) . What is the enthalpy fi atomisation of NH_(3)(g) ?. What is the avergae bond ethalpy of N-H bond?

If the end energies of H-H, Br-Br and H-Br are 433, 192 and 364 kJ mol^(-1) respectively, then DeltaH^(@) for the reaction, H_(2)(g)+Br_(2)(g)to2HB r(g) is

The rate of decomposition of NH_(3)(g) at 10 atm on platinum surface is zero order . What is rate of formation (in M min^(-1) ) of H_(2) (g) , if rate constant of reaction 2NH_(3(g)) to N_(2)(g) +3H_(2)(g) is 2.0 M min^(-1) ?

The values of heat of formation of SO_(2) and SO_(3) are - 298.2 kJ and - 98.2 kJ. The heat of reaction of the following reaction will be SO_(2)(g)+(1)/(2)O_(2)(g)to SO_(3)(g)