Question

why are some metallic oxides reduced by carbon and carbon monoxide while others are not?​

Answer 1

Question:-

why are some metallic oxides reduced by carbon and carbon monoxide while others are not?

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When coke or coal is used to reduce a metal oxide, it gets oxidized to CO. And, when CO itself is the reducing agent, it is oxidized to CO2 . ... Both thermodynamic and kinetic factors make carbon monoxide (CO) a better reducing agent than carbon. When coke or coal is used to reduce a metal oxide, it gets oxidized to CO

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Answer 2

Answer:

Libraries loan out books. When the patron has read the book, they return it to the library. This is similar to what happens with metals and their electrons. Metals are like the library, they give away electrons (books), and get the electrons (books) back in a reduction reaction. Let's pretend we are checking out a book on metallic oxide reduction to learn the details of this process.Before we get into oxidation and reduction, we have to discuss superscripts, which are numbers written above an element's symbol. For example, the +2 superscript in Zn+2 is the charge on the ion. There is no superscript on an element's symbol when it is not in a bond with another element because it is neutral. A compound will have multiple elements that have bonded. Each atom in the compound has a charge even though no superscripts are shown. Next, we will discuss the reactivity series.

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