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Characteristics of Equilibrium Constant

2SO2+O2⇌ 2SO3...

Question

$2 {S O}_{2} + O_{2} ⇌ 2 {S O}_{3}$ . Starting with $2$ mol ${S O}_{2}$ and $1 m o l$ $O_{2}$ in $1 L$ flask, mixture required $0.4 m o l$ $M n O_{4}^{-}$ in acidic medium. Hence $K_{c}$ is :

2

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Solution

The correct option is A $2$
$S O_{2} is oxidised by {M n O}_{4}^{-} is acidic medium$
$\begin{matrix} 6 {S O}_{2} & + 2 {M n O_{4}}^{-} \to 2 {M n}^{2 +} + 5 {S O}_{4}^{2 -} 2 m o l {M n O}_{4}^{-} = 5 m o l {S O}_{2} \end{matrix}$
$hence, 0.4 m o l {M n O}_{4}^{-} = 1 m o l {S O}_{2}$
$\begin{matrix} 2 {S O}_{2} + O_{2} ⇌ 2 {S O}_{3} 210 (2 - 2 x) (1 - x) 2 x \end{matrix}$
$\begin{matrix} (2 - 2 x) = 1 mol as determined by M n O_{4}^{2 -} \Rightarrow x = 0.5 \end{matrix}$
$\Rightarrow [S O_{3}] = \frac{2 K}{V} = 1 M (x = 0.5, V = 1)$
$\Rightarrow [S O_{2}] = \frac{2 - 2 x}{V} = 1 M$
$\begin{matrix} \Rightarrow [O_{2}] = \frac{1 - x}{V} = & 0.5 M K_{C} = \frac{{[S O_{3}]}_{3}^{2}}{{[{S O}_{2}]}_{2}^{2} [O_{2}]} = & \frac{1^{2}}{1^{2} \times 0.5} = 2 \end{matrix}$

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Similar questions

2 {S O}_{2} + O_{2} ⇌ 2 {S O}_{3}

starting with

2

mol of

{S O}_{2}

and

1

mol of

O_{2}

1

litre flask, mixture required

0.4

mol of

M n O_{4}^{-}

in acid medium. Hence

K_{c}

is:

2 S O_{2} + O_{2} ⇌ 2 S O_{3}

. Starting with

2

moles

S O_{2}

and

1

mole

O_{2}

1

L flask, mixture required

0.4

mole

M n O_{4}^{-}

in acidic medium. Hence, equilibirum constant

K

is:

Q. In a study of equilibrium

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

.
Starting with 2 mole

S O_{2}

and 1.5 mole

O_{2}

in 5 litre flask.Equilibrium mixture required 0.4 mole

K M n O_{4}

in acidic medium.Hence

K_{C}

is:

K_{c}

for

2 S O_{2} + O_{2} ⇌ 2 S O_{3}

in a

10 l i t

flask at certain

T

100 l i t . m o l^{- 1}

. Now , if equilibrium pressures of

S O_{2}

and

S O_{3}

are equal , then mass of

O_{2}

present at equilibrium is:

2 S O_{2} + O_{2} \to 2 S O_{3}

Rate of formation of

S O_{3}

according to the reaction is

1.6 \times 10^{- 3}

m i n^{- 1}

. Hence rate at which

S O_{2}

reacts is:

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2SO2+O2⇌2SO3. Starting with 2 mol SO2 and 1mol O2 in 1L flask, mixture required 0.4mol MnO−4 in acidic medium. Hence Kc is :

$2 {S O}_{2} + O_{2} ⇌ 2 {S O}_{3}$ . Starting with $2$ mol ${S O}_{2}$ and $1 m o l$ $O_{2}$ in $1 L$ flask, mixture required $0.4 m o l$ $M n O_{4}^{-}$ in acidic medium. Hence $K_{c}$ is :