Question

If enthalpy change for the reaction ocl2(g)----->o(g)+2cl(g) is 420kj per mol then average bond energy of "o-cl"bond will be...

Answer 1

Answer:

$210\frac{kj}{mol}$

Explanation:

The enthalpy of reaction is related to the bond energy as:

$enthalpyofreaction=[sumofbondenergyofreactants]-[sumofbondenergyofproducts]$

There is no bond involved on the product side as all the products are in atomic form.

$Enthalpyofreaction=[2XbondenergyO-Cl]-[0]=420$

$BondenergyofO-Cl=\frac{420}{2}=210\frac{kj}{mol}$

Answer 2

The average bond energy of "O-Cl"bond will be 210 kJ/mol.

Explanation:

$OCl2(g)\rightarrow O(g)+2Cl(g)$ , ΔH = 420 kJ/mol

In a given reaction , to break 2 single bonds of O-Cl we will need 420 kJ/mol in total.

Average bond energy of O-Cl bond = $\Delta H_{O-Cl}$

$\Delta H_{O-Cl}=\frac{\Delta H}{2}$

$=\frac{420 kJ/mol}{2}=210 kJ/mol$

The average bond energy of "O-Cl"bond will be 210 kJ/mol.

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