The following redox reaction occurs in an acidic solution- Ce4- - Bi - Ce3- - BiO- What is the coefficient before the Ce4- when the equation is fully balanced-

The correct option is B 3The unbalanced redox equation is #160; #160; Ce^4+ + Bi → Ce^3+ + BiO^+ The oxidation number of Ce decreases from +4 to +3. Th ...

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Byju's Answer

Standard XII

Chemistry

Oxidation Number Method

The following...

Question

The following redox reaction occurs in an acidic solution: $C e^{4 +} + B i \to C e^{3 +} + B i O^{+}$ . What is the coefficient before the $C e^{4 +}$ when the equation is fully balanced?

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Solution

The correct option is B 3
The unbalanced redox equation is
$C e^{4 +} + B i \to C e^{3 +} + B i O^{+}$
The oxidation number of Ce decreases from +4 to +3. The net decrease in the oxidation number is 1.
The oxidation number of Bi increases from 0 to +3. Net increases in the oxidation number is 3.
To balance increase in oxidation number with decrease in oxidation number, multiply the Ce species with 3.
$3 C e^{4 +} + B i \to 3 C e^{3 +} + B i O^{+}$
To balance O atoms, add one water molecule on left hand side.
$3 C e^{4 +} + B i + H_{2} O \to 3 C e^{3 +} + B i O^{+}$
To balance H atoms, add two protons on right hand side
$3 C e^{4 +} + B i + H_{2} O \to 3 C e^{3 +} + B i O^{+} + 2 H^{+}$
This is the fully balanced redox equation.
The coefficent before $C e^{4 +}$ is 3.

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Similar questions

For the given cell reaction:

F e^{2 +} + C e^{4 +} ⇌ F e^{3 +} + C e^{3 +}

. The equilibrium constant is:

(Given:

E_{{C e}^{4 +} / C e^{3 +}}^{\circ} = 1.44 V; E_{F e^{2 +} / F e^{3 +}}^{\circ} = 0.68 V

)

Q. Assertion :

C e^{4 +}

is good analytical reagent. Reason:

C e^{4 +}

has the tendency to change to

C e^{3 +}

Q. Calculate the equilibrium constant for the reaction

F e^{2 +} + C e^{4 +} ⇌ F e^{3 +} + C e^{3 +}

[Given:

E_{C e^{4 +} / C e^{3 +}}^{0} = 1.44 V; E_{F e^{3 +} / F e^{2 +}}^{0} = 0.68 V]

Q. Find the equilibrium constant for the reaction,

F e^{2 +} + C e^{4 +} ⇌ F e^{3 +} + C e^{3 +}

[Given:

E_{C e^{4 +} / C e^{3 +}}^{o} = 1.44 V; E_{F e^{3 +} / F e^{2 +}}^{o} = 0.68 V

]

Q. Balance the following equation by ion electron method.

H g_{2} (C N)_{2} + C e^{4 +} \to C O_{3}^{2 -} + N O_{3}^{-} + H g (O H)_{2} + C e^{3 +}

(basic medium).

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The following redox reaction occurs in an acidic solution: Ce4++Bi→Ce3++BiO+. What is the coefficient before the Ce4+ when the equation is fully balanced?

The following redox reaction occurs in an acidic solution: $C e^{4 +} + B i \to C e^{3 +} + B i O^{+}$ . What is the coefficient before the $C e^{4 +}$ when the equation is fully balanced?