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Biology and Chemistry Homework Help
Can Methane and Citric Acid be Balanced in a Redox Reaction?
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[QUOTE="Danny.Boy, post: 5508804, member: 454833"] Hi there: I'm trying to balance a reaction in which methane is oxidized by citric acid in solution. Both methane and citric acid will be transformed into carbon dioxide. To begin, I checked that the reaction is indeed a redox reaction. C[SUB]6[/SUB]H[SUB]8[/SUB]O[SUB]7[/SUB]→CO[SUB]2[/SUB] So, I calculated the oxidation number for carbon goes from +6 to +4. A reduction. CH[SUB]4[/SUB]→CO[SUB]2[/SUB] I calculated the oxidation number for carbon goes from -4 to +4. An oxidation. This seems reasonable so far. Then, I balanced my half-reactions. C[SUB]6[/SUB]H[SUB]8[/SUB]O[SUB]7[/SUB]+5H[SUB]2[/SUB]O→6CO[SUB]2[/SUB]+18H[SUP]+[/SUP]+18e[SUP]-[/SUP] CH[SUB]4[/SUB]+2H[SUB]2[/SUB]O→CO[SUB]2[/SUB]+8H[SUP]+[/SUP]+8e[SUP]-[/SUP] Now comes the part that has me baffled. How do I combine these half-reactions and not end up with loads of electrons since they are on the right hand side of both half-reactions?! Clearly, I've done something very wrong. Any help would be appreciated. [/QUOTE]
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Can Methane and Citric Acid be Balanced in a Redox Reaction?
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