What is the change in oxidation number of $Cr$ in the following redox reaction?
$3H_2O_2(aq) + Cr_2O_7^{2-}(aq) + 8H^+(aq) \rightarrow 3O_2(g) + 2Cr^{3+}(aq) + 7H_2O(l)$
$3H_2O_2(aq) + Cr_2O_7^{2-}(aq) + 8H^+(aq) \rightarrow 3O_2(g) + 2Cr^{3+}(aq) + 7H_2O(l)$
- A$+2$ to $+3$
- B$-2$ to $+3$
- C$+7$ to $+3$
- D$+6$ to $+3$
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From the given list,the number of compounds with $+4$ oxidation state of Sulphur is $ . . . . . . $.
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What are the oxidation numbers of the underlined elements in each of the following and how do you rationalise your results?
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$(b)$ $H_2\underline {S_4}O_6$
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$(a)$ $K\underline {I_3}$
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