The standard electrode potential ( M 3+ / M 2+) for V , Cr , Mn Co are -0.26 V, -0.41 V ,+1.57 V and +1.97 V, respectively. The metal ions which can liberate H 2 from a dilute acid are

Question

The standard electrode potential ( M 3+ / M 2+) for V , Cr , Mn Co are -0.26 V, -0.41 V ,+1.57 V and +1.97 V, respectively. The metal ions which can liberate H 2 from a dilute acid are (A) V 2+ and Mn 2+ (B) Mn 2+ and Co 2+ (C) Cr 2+ and Co 2+ (D) V 2+ and Cr 2+

Tardigrade Admin · Accepted Answer

Metal cation with (-) value of reduction potential ( M +3 / M +2) or with (+) value of oxidation potential ( M +2 / M +3) will liberate H 2 Therefore they will reduce H + i.eV +2 and Cr +2

Q. The standard electrode potential $(M^{3 +} / M^{2 +})$ for $V, C r, M n$ & Co are $- 0.26 V$ , $- 0.41 V, + 1.57 V$ and $+ 1.97 V$ , respectively. The metal ions which can liberate $H_{2}$ from a dilute acid are

$V^{2 +}$ and $M n^{2 +}$

$M n^{2 +}$ and $C o^{2 +}$

$C r^{2 +}$ and $C o^{2 +}$

$V^{2 +}$ and $C r^{2 +}$

Metal cation with $(-)$ value of reduction potential $(M^{+ 3} / M^{+ 2})$ or with $(+)$ value of oxidation potential $(M^{+ 2} / M^{+ 3})$ will liberate $H_{2}$
Therefore they will reduce $H^{+}$
i.eV $^{+ 2}$ and $C r^{+ 2}$

Q. The standard electrode potential (M3+/M2+) for V,Cr,Mn & Co are −0.26V, −0.41V,+1.57V and +1.97V, respectively. The metal ions which can liberate H2​ from a dilute acid are

V2+ and Mn2+

Mn2+ and Co2+

Cr2+ and Co2+

V2+ and Cr2+