It is easy to find home chemistry experiments for sodium peroxide but not so much sodium percarbonate. Industrially sodium percarbonate is used a sodium peroxide source- it is close enough to used as a substitute for common home experiments?

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    $\begingroup$ you really need to specify what experiment you want to do. $\endgroup$ Aug 10 at 2:38
  • $\begingroup$ Sorry my addled brain thought I was writing hydrogen peroxide $\endgroup$ Aug 10 at 7:05
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    $\begingroup$ Then fix it in the question title/body, otherwise readers will take it as the valid content. (Fixing it on the author behalf is always a risk not to match what the author has in mind .). // In the current question wording, the answer is it cannot be said until the particular scenario is specified. $\endgroup$
    – Poutnik
    Aug 10 at 8:18
  • $\begingroup$ It is not a true peroxoacid anion like persulphate or peracetate. It is a peroxohydrate, releasing free hydrogen peroxide when dissolved, or at contact with suitable solvent. $\endgroup$
    – Poutnik
    Aug 10 at 8:44

These behave fairly differently, in most cases. Look at the Safety Data Sheets, first:

$\ce{Na2O2}$ is a more powerful oxidizer, more likely to start combustion in contact with organic substances, can cause skin corrosion, and is generally not very stable.

$\ce{Na2CO3.1.5 H2O2}$ is a less powerful oxidizer, a bit more stable, less toxic orally, and is not listed as corrosive to skin (caustic), just possibly irritating.

Yes, both can be used as a source of oxygen, $\ce{O2}$, but $\ce{Na2O2}$ can react abruptly, perhaps causing a conflagrating explosion. In some use, the water and $\ce{CO2}$ that accompany evolution of oxygen from $\ce{Na2CO3.1.5 H2O2}$ might interfere with a reaction.

Caveat pharmacopolium: It is possible, if you have the chemical and engineering knowledge, to use one in place of the other in some situations... but you'd need to be specific to get any assurance.


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