For the following reaction
KClO–>KCl+1/2O2
assign oxidation states to each element on each side of the equation.
a. Reactants for K, Cl, and O
b. Products for K, Cl, O
c. Which element is oxidized?
d. Which element is reduced?
3 Answers
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+1+1-2…….+1-1………0
KClO(s) –> KCl(s) + ½O2(g)
O is oxidized
Cl is reduced
Oxidation is an increase in oxidation state, and reduction is a decrease in oxidation state. Oxygen is oxidized from -2 to zero, while chlorine is reduced from +1 to -1.
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Kcl 1
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RE:
For the following reaction
KClO–>KCl+1/2O2
assign oxidation states to each element on each side of the equation.?
For the following reaction
KClO–>KCl+1/2O2
assign oxidation states to each element on each side of the equation.
a. Reactants for K, Cl, and O
b. Products for K, Cl, O
c. Which element is oxidized?
d. Which element is reduced?
