Home
Class 12
CHEMISTRY
For Br2(l) Enthalpy of atomisation = x k...

For `Br_2(l)` Enthalpy of atomisation = x kJ/mol, Bond dissociation enthalpy of bromine = y kJ/mole, then

A

`x gt y`

B

`x lt y`

C

`x = y`

D

Relation does not exist

Text Solution

Verified by Experts

The correct Answer is:
A

NA
Promotional Banner

Similar Questions

Explore conceptually related problems

Use the following data to calculate Delta_("lattice") H^(@) for NaBr. Delta_("sub")H^(@) for sodium metal =108.4 kJ mol^(-1) , ionization enthalpy of sodium =496 kJ mol^(-1) ., electron gain enthalpy of bromine =-325 kJ mol^(-1) bond dissociation enthalpy of bromine =192 kJ mol^(-1) , Delta _f H^(@) for NaBr(s) - 360 kJ mol^(-1) .

Use the following data to calculate Delta_("lattice")H^(@) for NaBr. Delta_("sub")H^(@) for sodium metal = 108.4 kJ "mol"^(-1) .Ionization enthalpy of sodium = 496 kJ "mol"^(-1) Electron gain enthalpy of bromine = -325 kJ "mol"^(-1) .Bond dissociation enthalpy of bromine = 192 kJ "mol"^(-1) . Delta_(f)^(H^(@)) for NaBr (s) = -360.1 kJ "mol"^(-1) .

Calculate the lattice enthalpy of KCl from the following data by Born- Haber's Cycle. Enthalpy of sublimation of K = 89 kJ mol^(–1) Enthalpy of dissociation of Cl = 244 kJ mol^(–1) Ionization enthalpy of potassium = 425 kJ mol^(–1) Electron gain enthalpy of chlorine = –355 kJ mol^(–1) Enthalpy of formation of KCl = –438 kJ mol^(-1)

If enthalpy of atomisation for Br_((2(l))) is xKJ//mol bond enthalpy for Br_2 is Y KJ//mol , the relation between them :

From the following data : Enthalpy of formation of CH_(3)CN =87.86 kJ/mol Enthalpy of formation of C_(2)H_(6)=- 83.68 kJ/mol Enthalpy of sublimation of graphite =719.65 kJ/mol enthalpy of dissociation of nitrogen =945.58 kJ/mol Enthalpy of dissociation of H_(2) = 435.14 kJ/mol C-H bond enthalpy =414.22 kJ/mol Calculate the bond enthalpy of (i) C-C , (ii) C equiv N

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)

The enthalpy of dissociation (in kJ/mol) of fluorine, chlorine, bromine and iodine are :