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Grade upto college level Physical Chemistry

The enthalpy for the following reaction (∆Ho) at 25oC are given below :
(i) 1/2 H2(g) + 1/2 O2(g) → OH(g) 10.06 kcal
(ii) H2(g) → 2H(g) 104.18 kcal
(iii) O2(g) → 2O(g) 118.32 kcal
Calculate the O-H bond energy in the hydroxyl radical.

Profile image of Shane Macguire
12 Years agoGrade upto college level
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1 Answer

Profile image of Deepak Patra
12 Years ago
The required reaction in terms of dissociation energy is OH(g) → O(g) + H(g); ∆H = ?
This equation can be achieved by (a) reversing the equation (i), (b) dividing equation (ii) and (iii) each by 2, and (c) adding the three resulting equations.
OH(g) → 1/2 H2(g) + 1/2 O2(g); ∆H = + 10.06 kcal [Reversing eq (i)]
1/2 H2(g) → H(g);p ∆H = - 52.09 kcal [ 1/2 Eq (ii)]
OH(g) → O(g) + H(g); ∆H = - 101.19 kcal (adding)
Thus one mole of OH(g) needs 101.19 kcal of energy to break into oxygen and hydrogen gaseous atom. Hence the bond energy of O-H bond is 101.19 kcal.

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