|By Adr531 (Adr531) on Saturday, October 18, 2003 - 05:19 pm: Edit|
im studying for the AP chem and came across a question.
the following unbalanced equation represents a reaction that occurs in basic solution:
MnO4^(2-) +C2O4^(2-) ---->MnO2 +CO3^(2-)
how many moles of MnO4^(2-) are required to produce 1 mole of CO3^(2-)
|By Magoo112 (Magoo112) on Saturday, October 18, 2003 - 06:32 pm: Edit|
isn't the ratio between MnO4 and CO3 1:2???
|By Adr531 (Adr531) on Saturday, October 18, 2003 - 06:33 pm: Edit|
i thought so too but it cant be that easy. i have to figure out how to balance using oxidation/reduction...
|By Adr531 (Adr531) on Sunday, October 19, 2003 - 02:56 pm: Edit|
|By Silentopen (Silentopen) on Sunday, October 19, 2003 - 03:22 pm: Edit|
MnO4(2-) + C2O4(2-) ---> MnO2 + CO3(2-)
MnO4(2-) + C2O4(2-) ---> MnO2 + 2CO3(2-)
This equation has all non-oxygen and non-hydrogen elements balanced, oxygen balanced, and, finally, charge balanced. Therefore, no special redox balancing rules are needed and the ratio between MnO4(2-) and CO3(2-) is 1:2, as Magoo112 has said. This means that 0.5 mol of MnO4(2-) is required to produce 1 mol of CO3(2-).
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