How do you oxidize a formula?

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Emily Vainberg 1D
Posts: 102
Joined: Sat Jul 20, 2019 12:15 am

How do you oxidize a formula?

Postby Emily Vainberg 1D » Wed Oct 02, 2019 3:22 pm

For the hw problem L.7, part b asks, "What mass of oxygen is needed to oxidize this amount of tristearin?" Can someone explain how you would go about solving this problem?

Caitlyn Tran 2E
Posts: 100
Joined: Fri Aug 09, 2019 12:15 am

Re: How do you oxidize a formula?

Postby Caitlyn Tran 2E » Wed Oct 02, 2019 3:29 pm

Oxidation is just another word for combustion (burning) since combustion involves a substance reacting with oxygen to form carbon dioxide and water vapor. To solve part b of L.7, use dimensional analysis like you did for part a. However, instead of for every 2 mol of fat, there are 110 mol of H2O, put for every 2 mol of fat, there are 163 mol of O2. Then multiply by the molar mass of O2 to get the mass of oxygen needed to oxidize this amount of tristearin.

Sydney Myers 4I
Posts: 100
Joined: Fri Aug 09, 2019 12:17 am

Re: How do you oxidize a formula?

Postby Sydney Myers 4I » Wed Oct 02, 2019 4:36 pm

The previous reply is right; in this problem, all you need to know about oxidation is that it occurs during combustion. If you want to understand what oxidation is though, it is what happens when an atom loses some of its electrons during a chemical reaction. Oxygen has a high electronegativity, so when it reacts with other elements, it generally takes some of their electrons, and that's why we say "oxidized" or "oxidation."


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