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So I found these reduction potentials online:

$$\begin{alignat}{2} \ce{H2O2 + 2H+ + 2e- \;&<=> 2H2O}\qquad &&E=1.78\ \mathrm V\\ \ce{2Cl- \;&<=> Cl2 + 2e-}\qquad &&E=-1.36\ \mathrm V \end{alignat}$$

If the net reduction potential is positive will chlorine gas be spontaneously formed when salt and hydrogen peroxide are mixed in a acidic solution?

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    $\begingroup$ Exactly what is an acidic base...? Anyway, theoretically, yes. However kinetically the reaction may not be favoured. $\endgroup$ Dec 13, 2015 at 2:49

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Not necessarily. If you get the pH right and the stoichiometry absolutetly 1:1 then you might form $\ce{Cl2}$. However your reaction will compete with other reaction and you will more likely oxidize the chlorine into chlorate ions ($\ce{ClO-}$, $\ce{ ClO2-}$, $\ce{ClO3-}$, or $\ce{ClO4-}$).

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  • $\begingroup$ If you want to form chlorine I suggest calcium hypochlorite and hydrochloric acid or potassium permanganate and hydrochloric acid. $\endgroup$
    – A.K.
    Dec 13, 2015 at 15:22

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