The observed heat of formation of CH 3 COOH g is -439 kJ- The enthalpy of resonance of CH 3 COOH g is X kJ from the given data- Find the value of - X - Bond energy kJ Heat of atomizationkJ C - H -413C solid -716 C - C -348H 2-436 - C - O -732- C - O -351- O - H -463 -O 2-498

2C(s)+2H_2(g)+O_2 →without resonanceCH_3COOH(g) Δ H_f = (716 × 2) +(436× 2)+498 (413 ×3) 348 732 351 463 = 331 kJ CH_3COOH (without resonance) → CH_3COOH ...

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Byju's Answer

Standard XII

Chemistry

Reactions of Alkyl Halides

The observed ...

Question

The observed heat of formation of $C H_{3} C O O H (g)$ is -439 kJ. The enthalpy of resonance of $C H_{3} C O O H (g)$ is $X$ kJ from the given data. Find the value of $| X |$ .
$\begin{matrix} Bond energy (kJ) & Heat of atomization(kJ) C-H = 413 & C (solid)=716 C-C = 348 & H_{2} = 436 C=O = 732 & O_{2} = 498 C-O = 351 O-H = 463 \end{matrix}$

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Solution

$2 C (s) + 2 H_{2} (g) + O_{2} \to C H_{3} C O O H (g) without resonance$
$Δ H_{f} = (716 \times 2) + (436 \times 2) + 498 - (413 \times 3) - 348 - 732 - 351 - 463 = - 331 k J$
$C H_{3} C O O H (without resonance) \to C H_{3} C O O H (with resonance)$
$Δ H_{r e s o} = - 439 - (- 331) = - 108 k J$

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The observed heat of formation of CH3COOH(g) is -439 kJ. The enthalpy of resonance of CH3COOH(g) is X kJ from the given data. Find the value of |X|. Bond energy (kJ)Heat of atomization(kJ)C-H = 413C (solid)=716C-C = 348H2=436C=O = 732O2=498C-O = 351O-H = 463

2C(s)+2H2(g)+O2→CH3COOH(g)without resonance ΔHf=(716×2)+(436×2)+498−(413×3)−348−732−351−463=−331 kJ CH3COOH(without resonance)→CH3COOH (with resonance) ΔHreso=−439−(−331)=−108 kJ

$2 C (s) + 2 H_{2} (g) + O_{2} \to C H_{3} C O O H (g) without resonance$
$Δ H_{f} = (716 \times 2) + (436 \times 2) + 498 - (413 \times 3) - 348 - 732 - 351 - 463 = - 331 k J$
$C H_{3} C O O H (without resonance) \to C H_{3} C O O H (with resonance)$
$Δ H_{r e s o} = - 439 - (- 331) = - 108 k J$