For the following reaction KClO–>KCl+1/2O2 assign oxidation states to each element on each side of the equation.?

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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

  • +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.

  • 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?

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