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student101
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Why would hydrogen peroxide react better in the presence of magnesium dioxide than in the presence of sand? Also, in human systems, why is it good to have small particles rather than large chunks?
I don't think the first one counts as a catalyst question. Magnesium dioxide is a peroxide, so of course it's going to work better. Sand is not a peroxide, and it's very stable; it's so stable that it's basically inert.student101 said:Why would hydrogen peroxide react better in the presence of magnesium dioxide than in the presence of sand? Also, in human systems, why is it good to have small particles rather than large chunks?
The presence of magnesium can act as a catalyst, speeding up the reaction between hydrogen peroxide and other substances. It can also help to stabilize the reaction and make it more efficient.
Magnesium has a high surface area and a strong reactivity with hydrogen peroxide. This means that it can break down the hydrogen peroxide molecules more quickly, leading to a faster reaction rate.
Magnesium acts as a reducing agent, meaning it can donate electrons to the hydrogen peroxide molecules. This helps to break down the bonds in the hydrogen peroxide, causing it to decompose into water and oxygen gas.
Yes, other metals such as iron, nickel, and copper can also be used as catalysts in hydrogen peroxide reactions. However, magnesium is often preferred due to its high reactivity and lower cost.
Yes, the purity and particle size of magnesium can impact its effectiveness in hydrogen peroxide reactions. Finely ground magnesium with a high purity will provide a larger surface area for the reaction to occur, leading to a faster and more efficient reaction.