Home
Class 11
CHEMISTRY
The bond energy of H(2) is 104.3 k.cal m...

The bond energy of `H_(2)` is `104.3 k.cal mol^(-1)`. It means that

A

104.3K.cal heat is released during breaking up 'N' bonds in N molecules of `H_(2)`

B

104.3K.cal heat is needed to break up `6.023xx10^(23)` molecules into `1.2046xx10^(24)` atoms of H

C

104.3K.cal heat is evolved during combination of 2N atoms of H to form N molecules of `H_(2)`

D

Both 2 and 3

Text Solution

Verified by Experts

The correct Answer is:
D
Definition of bond enthalpy
Promotional Banner

Similar Questions

Explore conceptually related problems

The bond energy of H_(2) is 104.3 kcal mol^(-1) . If means that :

The dissociation energy of CH_(4)(g) is 360 kcal mol^(-1) and that of C_(2)H_(6)(g) is 620 kcal mol^(-1) . The C-C bond energy

The bond energy of an O -H bond is 109 K. cal "mole"^(-1) . When a mole of water is formed

Bond dissociation energy of O_(2)(g) is x k J mol^(-1) . This means that

The average energy required to break a P-P bond in P_(4)(s) into gaseous atoms is 53.2 kcal mol^(-1) . The bond dissociation energy of H_(2)(g) is 104.2kcal mol^(-1) , Delta H_(f)^(0) of PH_(3)(g) from P_(4)(s) is 5.5 kcal mol^(-1) . The P-H bond energy in kcal mol^(-1) is [ Neglect presence of Van der Waals force in P_(4)(s) ]

Delta H_(1)C_(2)H_(4) = 12.5 kcal Heat of atomisation of C = 171 Kcal Bond energy of H_(2) = 104.3 kcal Bond energy C - H = 99.3 kcal What is C = C bond energy?

The enthalpy of formation of UF(g) is 22kcal mol^(-1) and that of U(g) is 128kcal mol^(-1) . The bond energy of the F-F bond is 37kcal mol^(-1) . The bond dissociation energy of UF(g) is (are):