Jen asked in Science & MathematicsChemistry · 3 weeks ago

Redox reaction?

There are 3 equation

1) 2ZnS(s)+3O2(g)-->2ZnO(s)+2SO2(g)

2) Ag+(aq)+Br-(aq)-->AgBr(s)

3) 10H+(aq)+SO42-(aq)+8I-(aq)-->4I2(s)+H2S(g)+4H2O(l)

classify each reactant in the chemical equations as an Oxidizing agent, Reduced agent, or neither.

ZnS

O2

Ag+

Br-

SO4^2-

I-

H+

Calculate the increase or decrease in oxidation state for ea. element listed as it changes from a reactant to a product.(Use a negative sign to show a decrease in oxidation state.)

Sulfur, beginning in the reactant ZnS

Bromine, beginning in the reactant Br-

Iodine, beginning in reactant I-

Sulfur, beginning in the reactant SO4^2-

I have been unsuccessful for over 2weeks, someone, please explain it to me.

1 Answer

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  • 3 weeks ago
    Favorite Answer

    Redox reactions .... oxidation state change.

    Oxidation is the increase in oxidation state.

    Reduction is the decrease in oxidation state.

    The oxidizing agent is the reactant which causes the oxidation, and contains the element reduced.

    The reducing agent is the reactant which causes the reduction, and contains the element oxidized.

    Start by assigning the oxidation state of each element, and the what changes.

    .... +2-2...........0 .............+2-2 ........ +4-2

    1) 2ZnS(s) + 3O2(g) --> 2ZnO(s) + 2SO2(g)

    Sulfur is oxidized, ZnS is the reducing agent

    Oxygen is reduced, O2 is the oxidizing agent

    2) Ag+(aq) + Br-(aq) --> AgBr(s) ..... not redox

    ....... +1.......... +6-2............... -1.............. 0 ........ +1-2......... +1-2

    3) 10H+(aq) + SO4^2-(aq) + 8I-(aq) --> 4I2(s) + H2S(g) + 4H2O(l)

    Iodine is oxidized, I- is the reducing agent

    Suflur is reduced , sulfate ion is the oxidizing agent

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