Question
I'm a bit iffy on oxidation numbers... can someone please tell me if this is correct?
Assign oxidation states to each element on both sides of the equation : KClO2--->KCl+O2
Reactants
K = +1
Cl = +1
O = -2
Products
K = +1
Cl = -1
O = 0
the element being reduced is Cl and the element being oxidized is Oxygen... is that correct?
Assign oxidation states to each element on both sides of the equation : KClO2--->KCl+O2
Reactants
K = +1
Cl = +1
O = -2
Products
K = +1
Cl = -1
O = 0
the element being reduced is Cl and the element being oxidized is Oxygen... is that correct?
Answers
products ok.
reactants:
K is +1
O is -2 EACH for a total of -4.
Therefore, Cl must be +3 to make KClO2 zero.
K2Cr2O7
K is +1
Cr is +6 each
O is -2 each
Total + = (2*1) +(2*6) = 14
Total - = 7*-2 = -14
reactants:
K is +1
O is -2 EACH for a total of -4.
Therefore, Cl must be +3 to make KClO2 zero.
K2Cr2O7
K is +1
Cr is +6 each
O is -2 each
Total + = (2*1) +(2*6) = 14
Total - = 7*-2 = -14
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