When the ion $C r_{2} O_{7}^{- 2}$ acts as an oxidant in acidic aqueous solution the ion $C r^{3 +}$ is formed. How many mole of $S n^{2} +$ would be oxidized to $S n^{4 +}$ by 2/3 moles of $C r_{2} O_{7}^{- 2}$ ions?

2 / 3

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Solution

The correct option is A $2 / 3$
The complete balanced oxidation reaction of ${S n}^{+ 2}$ with ${C r}_{2} O_{7}^{- 2}$ is.
${S n}^{+ 2} + {C r}_{2} O_{7}^{- 2} + 14 H^{+} ⟶ 3 {S n}^{+ 4} + 2 {C r}^{+ 3} + 2 K^{+} + 7 H_{2} O$
By this balanced one molecule/ion of ${S n}^{+ 2}$ requires one ion ${C r}_{2} O_{7}^{- 2}$ to oxidise to ${S n}^{+ 4}$ then $2 / 3$ moles of ${S n}^{+ 2}$ requires $2 / 3$ moles of ${C r}_{2} O_{7}^{- 2}$ .
Ans :- Option A.

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Similar questions

When the ion ${C r}_{2} O_{7}^{2 -}$ acts as an oxidant in acidic aqueous solution the ion ${C r}^{3 +}$ is formed. How many moles of ${S n}^{2 +}$ would be oxidised to ${S n}^{4 +}$ by one mole of ${C r}_{2} O_{7}^{2 -}$ ions?

Q. Balance by Ion electon method,

C r_{2} O_{7}^{- 2} + F e^{+ 2} \to C r^{+ 3} + H_{2} O

(in acidic medium).

Q. The number of moles of oxalate ions oxidized by one mole of

M n O_{4}^{-}

ion in acidic medium.

Q. Number of moles of

C r_{2} O_{7}^{- 2}

required to oxidise one mole of ferrous ion completely in acidic medium.

Q. In acidic medium

C r_{2} O_{7}^{- 2}

is an oxiding agent

C r_{2} O_{7}^{- 2} + 14 H^{+} + 6 e^{-} \leftarrow 2 C r^{+ 3} + 7 H_{2} O

[E_{C r_{2} O_{7}^{- 2} / C r^{+ 3}}^{^{\circ}} = 1.33 V]

The electrode potential of half cell at

p H = 1

keeping concentration of other species unity is:

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When the ion Cr2O−27 acts as an oxidant in acidic aqueous solution the ion Cr3+ is formed. How many mole of Sn2+ would be oxidized to Sn4+ by 2/3 moles of Cr2O−27 ions?

The correct option is A 2/3The complete balanced oxidation reaction of Sn+2 with Cr2O−27 is.Sn+2+Cr2O−27+14H+⟶3Sn+4+2Cr+3+2K++7H2OBy this balanced one molecule/ion of Sn+2 requires one ion Cr2O−27 to oxidise to Sn+4 then 2/3 moles of Sn+2 requires 2/3 moles of Cr2O−27.Ans :- Option A.

When the ion $C r_{2} O_{7}^{- 2}$ acts as an oxidant in acidic aqueous solution the ion $C r^{3 +}$ is formed. How many mole of $S n^{2} +$ would be oxidized to $S n^{4 +}$ by 2/3 moles of $C r_{2} O_{7}^{- 2}$ ions?