H2O2 decomposes in an aqueous solution to give H2O and oxygen gas. The rate constant of disappearance is 2×10−2sec−1. Calculate the amount of heat liberated per second initially from 0.5 L of 2M H2O2 solution (in kJ)H2O2(aq)⟶H2O(l)+12O2(g)ΔH=−100kJ/mole

Given,ΔH=−100kJ/moleRate constant k=2×10−2sec−1Thus, the heat liberated per second,Q=2×10−2×1×100 Q=2kJ

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$H_{2} O_{2}$ decomposes in an aqueous solution to give $H_{2} O$ and oxygen gas. The rate constant of disappearance is $2 \times 10^{- 2} \sec^{- 1}$ . Calculate the amount of heat liberated per second initially from 0.5 L of 2M $H_{2} O_{2}$ solution (in kJ)
$H_{2} O_{2} (aq) ⟶ H_{2} O (l) + \frac{1}{2} O_{2} (g)$
$ΔH = - 100 kJ / mole$

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Detailed Solution

Given,

$ΔH = - 100 kJ / mole$

Rate constant $k =$ $2 \times 10^{- 2} \sec^{- 1}$

Thus, the heat liberated per second,

$Q = 2 \times 10^{- 2} \times 1 \times 100 Q = 2 kJ$

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