The average O-H bond energy with the help of following data is-1 2 H g - H 2 g - - H -435-0 kJ mol -12 O 2 g - 2 O g - - H -489-6 kJ mol -13 1-2 H 2 g -1-2 O 2 g - OH - - H -42-09 kJ mol -1A- 584-9 kJ mol -1B- 279-8 kJ mol -1C- 420 kJ mol -1D- 925 kJ mol -1

The correct option is C 420 kJ mol^ 1Required equation: ( 4) OH → O + H ;Δ H = nbsp; ? kJ mol^ 1 The above equation can be obtained as follows: 12eqn(2) ...

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Standard X

Physics

Specific Heat Capacity

The average O...

Question

The average O-H bond energy with the help of following data is:

$(1) 2 H (g) ⟶ H_{2} (g); Δ H = - 435.0 {kJ mol}^{- 1}$

$(2) O_{2} (g) ⟶ 2 O (g); Δ H = + 489.6 {kJ mol}^{- 1}$

$(3) \frac{1}{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ O H; Δ H = - 42.09 {kJ mol}^{- 1}$

584.9 {kJ mol}^{- 1}

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279.8 {kJ mol}^{- 1}

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420 {kJ mol}^{- 1}

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925 {kJ mol}^{- 1}

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Solution

The correct option is C $420 {kJ mol}^{- 1}$
Required equation:
$(4) O H \to O + H; Δ H = ? {kJ mol}^{- 1}$

The above equation can be obtained as follows:
$\frac{1}{2} e q n (2) - \frac{1}{2} e q n (1) - e q n (3) = e q n (4)$

Hence, the enthalpy can also be obtained similiarly.
$244.8 + 217.5 - 42 = 420 {kJ mol}^{- 1}$

Hence, the bond energy of $O H = 420 {kJ mol}^{- 1}$

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Similar questions

Q. The enthalpies for the following reactions at

25^{o} C

are given:

\frac{1}{2} H_{2} (g) + \frac{1}{2} O_{2} (g) \to O H (g); Δ H = 10.06 k c a l

H_{2} (g) \to 2 H (g); Δ H = 104.18 k c a l

O_{2} (g) \to 2 O (g); Δ H = 118.32 k c a l

Calculate the

O - H

bond energy in the

O H

group.

The enthalpies for the following reactions at 25°C are given.
$\frac{1}{2} H_{2} (g) + \frac{1}{2} O_{2} (g) \to O H (g); △ H = 10.06 K c a l$
$H_{2} (g) \to 2 H (g); △ H = 104.18 K c a l$
$O_{2} (g) \to 2 O (g); △ H = 118.32 K c a l$

Calculate the OH bond energy in the O - H group

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 H_{2} O (l); Δ H = - 86 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) . . . . . . . . . k J (\pm ?)

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 H_{2} O (l); Δ H = - 286 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l) . . . . . . . . . k J (\pm ?)

Q. From the following data at

25^{\circ} C

Reaction	$Δ_{r} H^{\circ}$ kJ/mol
$\frac{1}{2} H_{2} (g) + \to \frac{1}{2} O_{2} (g)$	$+ 42$
$H_{2} (g) + \frac{1}{2} O_{2} (g) H_{2} O (g)$	$- 242$
$H_{2} (g) \to 2 H (g)$ $O_{2} (g) \to 2 O (g)$	$+ 436$ $+ 495$

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The average O-H bond energy with the help of following data is: (1) 2H(g)⟶H2(g) ;ΔH=−435.0 kJ mol−1 (2) O2(g)⟶2O(g) ;ΔH=+ 489.6 kJ mol−1 (3) 12H2(g)+12O2(g)⟶OH ;ΔH=−42.09 kJ mol−1

The correct option is C 420 kJ mol−1Required equation: (4) OH→O+H ;ΔH=? kJ mol−1 The above equation can be obtained as follows: 12eqn(2)−12eqn(1)−eqn(3)=eqn(4) Hence, the enthalpy can also be obtained similiarly. 244.8+217.5−42=420 kJ mol−1 Hence, the bond energy of OH=420 kJ mol−1

The average O-H bond energy with the help of following data is:

$(1) 2 H (g) ⟶ H_{2} (g); Δ H = - 435.0 {kJ mol}^{- 1}$

$(2) O_{2} (g) ⟶ 2 O (g); Δ H = + 489.6 {kJ mol}^{- 1}$

$(3) \frac{1}{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ O H; Δ H = - 42.09 {kJ mol}^{- 1}$