Acidified potassium dichromate is treated with hydrogen sulphide. In the reaction, the oxidation number of chromiumIncreases from +3 to +6Decreases from +6 to +3Remains unchangedDecreases from +6 to +2
Question
Acidified potassium dichromate is treated with hydrogen sulphide. In the reaction, the oxidation number of chromiumIncreases from +3 to +6Decreases from +6 to +3Remains unchangedDecreases from +6 to +2
Solution
The oxidation number of chromium decreases from +6 to +3 in this reaction.
Here's the step by step explanation:
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Potassium dichromate (K2Cr2O7) is an orange compound where the oxidation state of chromium is +6.
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When acidified potassium dichromate is treated with hydrogen sulphide (H2S), the dichromate ion (Cr2O7^2-) is reduced to chromium (III) ion (Cr^3+).
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The balanced chemical equation for this reaction is: 3H2S + K2Cr2O7 + 4H2O = 2KHSO4 + 2Cr(OH)3 + 3S
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In this reaction, the oxidation state of chromium changes from +6 in the dichromate ion to +3 in the chromium (III) ion.
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Therefore, the oxidation number of chromium decreases from +6 to +3 in this reaction.
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