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Standard XII

Chemistry

Types of Redox Reactions

500 ml of 0.1...

Question

500 ml of 0.150 M $A g N O_{3}$ solution is mixed with 500 ml of 1.09 M $F e^{2 +}$ solution and the reaction is allowed to reach equilibrium at 300K $F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g$ For 25 ml of solution , 30 ml of 0.833 M $K M n O_{4}$ were required for oxidation.
Calculate the equilibrium constant for reaction at 300 K.

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Solution

The correct option is A 3
Initial no of mmoles $A g^{+}$ and $F e^{2 +}$ are 75 and 545 respectively
Now let x mmoles of the reactant consumed at equilibrium then 545-x mmoles of $F e^{2 +}$ are left and only it will be oxidized
for 25 ml of such solution $\frac{545 - x}{1000} \times 25 = 30 \times 0.0833 \times 5$
hence x = 45 mmol
$K_{c} = \frac{45 \times 1000}{30 \times 500} = 3$

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Similar questions

Q. 500 ml of 0.150 M

A g N O_{3}

solution is mixed with 500 ml of 1.09 M

F e^{2 +}

solution and the reaction is allowed to reach equilibrium at 300K

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

For 25 ml of solution , 30 ml of 0.833 M

K M n O_{4}

were required for oxidation.
Calculate the equilibrium constant for reaction at 300 K.

Q. To 500 mL of 0.150 M

{A g N O}_{3}

solution were added 500 mL of 1.09 M

{F e}^{+ 2}

solution and the reaction is allowed to reach an equilibrium at 25C.

{A g}^{\oplus} (a q) + {F e}^{+ 2} (a q) ⇌ {F e}^{+ 3} (a q) + A g (s)

For 25 mL of the solution, 30 mL of 0.0832 M

{K M n O}_{4}

was required for oxidation. Calculate the equilibrium constant for the reaction 25C.

Q. To

500 m L

0.150 M A g N O_{3}

solution were added

500 m L

1.09 M {F e}^{2 +}

solution and the reaction is allowed to reach an equilibrium at

25

{A g}^{+} (a q) + {F e}^{2 +} (a q) ⇌ {F e}^{3 +} (a q) + A g (s)

For

25 m L

of the solution,

30 m L

0.0832 M K M n O_{4}

were required for oxidation. The equilibrium constant for the reaction at

25

^{o} C

is_________.

Q. The amount of

M g

required to replace

A g

from 500 ml of 0.5 M

A g N O_{3}

solution is:

Q. At equimolar concentrations of

F e^{2 +}

and

F e^{3 +}

, what must

[A g^{+}]

be so that the voltage of the galvanic cell made from

A g^{+} / A g

and

F e^{3 +} / F e^{2 +}

electrodes equals zero? The reaction is

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

. Determine the equilibrium constant at

25^{\circ} C

for the reaction. (Given:

E_{A g^{+} / A g}^{\circ} = 0.799 v o l t

and

E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.771 v o l t

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500 ml of 0.150 M AgNO3 solution is mixed with 500 ml of 1.09 M Fe2+ solution and the reaction is allowed to reach equilibrium at 300K Fe2++Ag+⇌Fe3++Ag For 25 ml of solution , 30 ml of 0.833 M KMnO4 were required for oxidation. Calculate the equilibrium constant for reaction at 300 K.