- #1

Mk

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- Thread starter Mk
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- #1

Mk

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- #2

GCT

Science Advisor

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Find the reduction potential for the anions and compare.

- #3

Mk

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- #4

GCT

Science Advisor

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From what I remember, the more positive the potential, the better the oxidizing agent.

- #5

Mk

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- #6

Kushal

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i have some standard electrode values.

OCl[tex]^{-}_{(aq)}[/tex] + H[tex]^{+}_{(aq)}[/tex] + e[tex]^{-}[/tex] [tex]\Leftrightarrow[/tex] [tex]\frac{1}{2}[/tex]Cl[tex]_{2(aq)}[/tex] + 2H[tex]_{2}[/tex]O[tex]_{(l)}[/tex]

emf = + 1.64 V

NO[tex]^{-}_{3(aq)}[/tex] + 3H[tex]^{+}_{(aq)}[/tex] + 2e[tex]^{-}[/tex] [tex]\Leftrightarrow[/tex] HNO[tex]_{2(aq)}[/tex] + H[tex]_{2}[/tex]O[tex]_{(l)}[/tex]

emf = + 0.94 V

therefore, the chlorate(1) is a stronger oxidising agent.

OCl[tex]^{-}_{(aq)}[/tex] + H[tex]^{+}_{(aq)}[/tex] + e[tex]^{-}[/tex] [tex]\Leftrightarrow[/tex] [tex]\frac{1}{2}[/tex]Cl[tex]_{2(aq)}[/tex] + 2H[tex]_{2}[/tex]O[tex]_{(l)}[/tex]

emf = + 1.64 V

NO[tex]^{-}_{3(aq)}[/tex] + 3H[tex]^{+}_{(aq)}[/tex] + 2e[tex]^{-}[/tex] [tex]\Leftrightarrow[/tex] HNO[tex]_{2(aq)}[/tex] + H[tex]_{2}[/tex]O[tex]_{(l)}[/tex]

emf = + 0.94 V

therefore, the chlorate(1) is a stronger oxidising agent.

Last edited:

- #7

lightarrow

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Chlorate isi have some standard electrode values.

OCl[tex]^{-}_{(aq)}[/tex] + H[tex]^{+}_{(aq)}[/tex] + e[tex]^{-}[/tex] [tex]\Leftrightarrow[/tex] [tex]\frac{1}{2}[/tex]Cl[tex]_{2(aq)}[/tex] + 2H[tex]_{2}[/tex]O[tex]_{(l)}[/tex]

emf = + 1.64 V

NO[tex]^{-}_{3(aq)}[/tex] + 3H[tex]^{+}_{(aq)}[/tex] + 2e[tex]^{-}[/tex] [tex]\Leftrightarrow[/tex] HNO[tex]_{2(aq)}[/tex] + H[tex]_{2}[/tex]O[tex]_{(l)}[/tex]

emf = + 0.94 V

therefore, the chlorate(1) is a stronger oxidising agent.

[tex]ClO_3^{-}[/tex]

not

[tex]ClO^{-}[/tex]

- #8

Kushal

- 438

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oooops... yeah it is ClO3-

- #9

Mk

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Does this mean it is 1.7x stronger?emf = + 1.64 V

emf = + 0.94 V

therefore, the chlorate(1) is a stronger oxidising agent.

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