Use Fe = 56, S = 32, O = 16. A solution contains 0.02 mol KMnO4 and 0.01 mol K2Cr2O7 acidified with H2SO4. The mass of FeSO4 (to Fe^3+) that this oxidant mixture can oxidise completely (to Mn^2+ and Cr^3+) is:

JEE Advanced levelSingle correct optionDifficulty 3 of 3rx150

Use Fe = 56, S = 32, O = 16. A solution contains $0.02$ mol $KMnO X_{4}$ and $0.01$ mol $K X_{2} Cr X_{2} O X_{7}$ acidified with $H X_{2} SO X_{4}$ . The mass of $FeSO X_{4}$ (to $Fe X^{3 +}$ ) that this oxidant mixture can oxidise completely (to $Mn X^{2 +}$ and $Cr X^{3 +}$ ) is:

Equivalents of oxidants:

0.02 \times 5 + 0.01 \times 6 = 0.16

. Equal equivalents of

FeSO X_{4}

(

n = 1

)

= 0.16

mol. Mass

= 0.16 \times 152 = 24.32 g