Reaction Mg (s) with NaCl+H2O2+KOH solution

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When magnesium is inserted into a solution of NaCl, H2O2, and KOH, a reaction occurs that involves the oxidation of magnesium. The presence of H2O2 suggests it acts as an oxidizing agent, potentially leading to the formation of magnesium hydroxide and hydrogen gas. The KOH contributes to the alkaline environment, facilitating the reaction. Sodium chloride remains largely unreactive in this context. Understanding the roles of each component is crucial for predicting the products formed in this reaction.
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Homework Statement


I just want to know what reaction occurs when magnesium is inserted into NaCl+H2O2+KOH solution.

Homework Equations


What happened with each component in that solution ?

I would be very grateful if you could help me.

The Attempt at a Solution

 
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What have you observed?
 
Think of what role ##H_2 O_2## might be playing in the given reaction, it will give you an idea about the products formed.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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