1 lit $H 2 O 2$ solution having 1M concentration was left open causing first order decay of $H 2 O 2$ with rate constant equal to $6.93 × 10 − 2 sec − 1$ . If after 20 sec, the solution is reacted with excess of $I − (aq)$ forming $I 2 (g)$ with water then calculate the amount of energy released in kJ.
[Assume no change in volume of $H 2 O 2$ solution]
Given Data : $ΔH f ∘ H 2 O 2 aq = − 200 kJ / mole; ΔH f 0 I aq = − 60 kJ / mole$
$ΔH f 0 I 2 g = 60 kJ / mole; ΔH f 0 H 2 O = − 290 kJ$

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$K = \frac{2.303}{t} x \log \frac{a}{a - x}$

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