Mock Test 1 — Redox Reactions

ON of N in $HNO_3$:

The oxidizing agent in: $Cu + 2AgNO_3 \to Cu(NO_3)_2 + 2Ag$:

In acidic medium, $MnO_4^-$ converts to:

Strongest reducing agent in halogens:

ON of Cr in $CrO_5$ (peroxide complex, where 4 O are peroxide $-1$ and 1 is $-2$):

Equivalent weight of HCl:

The change in ON in $Cr_2O_7^{2-} \to 2Cr^{3+}$ (per molecule):

Element which never undergoes disproportionation:

In a redox reaction, oxidizing agent:

The number of moles of $K_2Cr_2O_7$ needed to oxidize $1$ mole of $Fe^{2+}$ in acidic medium:

$n$-factor of $K_2Cr_2O_7$ in acidic medium:

ON of Mn in $MnO_4^-$:

In $2KMnO_4 + 16HCl \to 2KCl + 2MnCl_2 + 5Cl_2 + 8H_2O$: moles of Cl₂ produced per mole of KMnO₄:

Assertion (A): $H_2O_2$ can act as both oxidizing and reducing agent. Reason (R): Oxygen in $H_2O_2$ has intermediate oxidation state ($-1$), so it can go to either $-2$ or $0$.

Assertion (A): Fluorine cannot undergo disproportionation. Reason (R): Fluorine exists only in $-1$ and $0$ oxidation states; it does not exhibit positive oxidation states.