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anonymous
 one year ago
half equation : C2H4 > C2H6O2
anonymous
 one year ago
half equation : C2H4 > C2H6O2

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taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2So I'm assuming you need help balancing this The first step is to add oxygen to balance out the oxygen on each side to do this you have to add H2O Then you have too many hydrogens on one side to balance it out you put hydrogen ions on the side that needs them The last step is to balance out the charges by adding electrons to the side that is more positive so they have the same charge on each side

arindameducationusc
 one year ago
Best ResponseYou've already chosen the best response.0@taramgrant0543664 for acidic and basic reactions, the process the different, right?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.2Yes @arindameducationusc the process is a little different depending on if it's under acidic or under basic conditions normally it says which one it is too Here are the rules I think I have it all: Under acidic conditions: Step 1: Write the skeletons of the oxidation and reduction halfreactions. (The skeleton reactions contain the formulas of the compounds oxidized and reduced, but the atoms and electrons have not yet been balanced.) See Example. Step 2: Balance all elements other than H and O. Step 3: Balance the oxygen atoms by adding H2O molecules where needed. Step 4: Balance the hydrogen atoms by adding H+ ions where needed. Step 5: Balance the charge by adding electrons, e. Step 6: If the number of electrons lost in the oxidation halfreaction is not equal to the number of electrons gained in the reduction halfreaction, multiply one or both of the half reactions by a number that will make the number of electrons gained equal to the number of electrons lost. Step 7: Add the 2 halfreactions as if they were mathematical equations. The electrons will always cancel. If the same formulas are found on opposite sides of the halfreactions, you can cancel them. If the same formulas are found on the same side of both halfreactions, combine them. Step 8: Check to make sure that the atoms and the charges balance. Under basic conditions: Steps 17: Begin by balancing the equation as if it were in acid solution. If you have H+ ions in your equation at the end of these steps, proceed to Step 8. Otherwise, skip to Step 11. Step 8: Add enough OH− ions to each side to cancel the H+ ions. (Be sure to add the OH− ions to both sides to keep the charge and atoms balanced.) Step 9: Combine the H+ ions and OH− ions that are on the same side of the equation to form water. Step 10: Cancel or combine the H2O molecules. Step 11: Check to make sure that the atoms and the charge balance. If they do balance, you are done. If they do not balance, recheck your work in Steps 110.

arindameducationusc
 one year ago
Best ResponseYou've already chosen the best response.0Nice work @taramgrant0543664 ....
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