Chemistry - Redox Reactions Question with Solution | TestHub

The same mass of H₂O₂ supplies the same number of g-eq (say 1 eq) in each experiment. KMnO₄ (n = 5): 0.2 mol = 31.6 g. K₂Cr₂O₇ (n = 6): 1/6 mol = 49 g. So mass of K₂Cr₂O₇ is greater (a true) while moles of KMnO₄ (0.2) exceed those of K₂Cr₂O₇ (0.167) (b true). Since H₂O₂ is the only source of O₂ in both, equal g-eq of H₂O₂ evolve equal masses of O₂ (c true). Equal volumes reacting completely means equal g-eq, i.e. equal normalities: 5M₁ = 6M₂, so M(KMnO₄):M(K₂Cr₂O₇) = 6:5 (d true). All four.