Redox and Equivalent ConceptHard

Question

A metal exhibits the valencies of 2 and 3. Its equivalent weight is 28 when it forms a metal oxide of formula MO. What mass of H2SO4 is needed for complete reaction with 4.8 g of M2O3?

Options

A.8.82 g
B.4.41 g
C.13.23 g
D.11.03 g

Solution

$28 = \frac{A_{M}}{2} \Rightarrow$Atomic mass of metal, AM = 56.

Now, neqH2SO4 = neqM2O3

Or $\frac{w}{98} \times 2 = \frac{4.8}{160} \times 6 \Rightarrow w = 8.82g$

Create a free account to view solution

View Solution Free
Topic: Redox and Equivalent Concept·Practice all Redox and Equivalent Concept questions

More Redox and Equivalent Concept Questions

Which of the following ion cannot act as an oxidizing agent?...The specific conductance (κ) of an electrolyte of 0.1 N concentration is related to equivalent conductance (Λe...The number of moles of Cr2O72− needed to oxidize 0.136 equivalent of N2H5+ through the reactionN2H5+ + Cr2O72− → N2 + Cr...The equivalent weight of H2SO4 in the reaction: 2KMnO4 + 3H2SO4 + 10HCl → 2MnSO4 + K2SO4 + 5Cl2 + 8H2O, is...An ion is reduced to the element when it absorbs 6 × 1020 electrons. The number of equivalents of the ion is...