Question
A definite mass of H2O2 is oxidized by excess of acidified KMnO4 and acidified K2Cr2O7 in separate experiments. Which of the following is/ are correct statements? (K = 39, Cr = 52, Mn = 55)
Options
Solution
$n_{eq}H_{2}O_{2} = n_{eq}KMnO_{4} = n_{eq}K_{2}Cr_{2}O_{7} = n_{eq}O_{2}$
$\text{Or }\text{n}_{KMnO_{4}} \times 5 = n_{K_{2}Cr_{2}O_{7}} \times 6 $$$\Rightarrow n_{KMnO_{4}} > n_{K_{2}Cr_{2}O_{7}}$$
$\text{Or }\frac{W_{KMnO_{4}}}{158} \times 5 = \frac{W_{K_{2}Cr_{2}O_{7}}}{294} \times 6 $$${\Rightarrow W_{KMnO_{4}} < W_{K_{2}Cr_{2}O_{7}} }{\text{Or }\frac{V \times M_{KMnO_{4}}}{1000} \times 5 = \frac{V \times M_{K_{2}Cr_{2}O_{7}}}{1000} \times 6 }{\Rightarrow \frac{M_{KMnO_{4}}}{M_{K_{2}Cr_{2}O_{7}}} = \frac{6}{5}}$$
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