In the reaction of formation of sulphur trioxide by contact process- 2SO2 - O2 -2SO3- the rate of reaction was measured as d-O2-dt-2-5 - 10-4mol L-1s-1- The rate of disappearance of -SO2- in mol-L-1s-1 will be-

The correct option is B 5.00 × 10^ 4 Given that, 2SO_2 + O_2 ⇌2SO_3 Now, d[O_2]dt=d[SO_2]2× dt= 2.5 × 10^ 4 mol .L^ 1s^ 1 d[SO_2]dt= 5 × 10^ ...

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Byju's Answer

Standard XII

Chemistry

Reaction Quotient

In the reacti...

Question

In the reaction of formation of sulphur trioxide by contact process; $2 S O_{2} + O_{2} ⇌ 2 S O_{3}$ , the rate of reaction was measured as $\frac{d [O_{2}]}{d t} = - 2.5 \times 10^{- 4} m o l L^{- 1} s^{- 1}$ . The rate of disappearance of $[S O_{2}]$ in $m o l . L^{- 1} s^{- 1}$ will be:

- 3.75 \times 10^{- 4}

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- 1.25 \times 10^{- 4}

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- 2.50 \times 10^{- 4}

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- 5.00 \times 10^{- 4}

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Solution

The correct option is B $- 5.00 \times 10^{- 4}$
Given that,

$2 S O_{2} + O_{2} ⇌ 2 S O_{3}$

Now,

$\frac{d [O_{2}]}{d t} = \frac{d [S O_{2}]}{2 \times d t} = - 2.5 \times 10^{- 4} m o l . L^{- 1} s^{- 1}$
$\frac{d [S O_{2}]}{d t} = - 5 \times 10^{- 4} m o l . L^{- 1} s^{- 1}$

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Similar questions

Q. In the formation of sulphur trioxide by contact process,

2 S O_{2} + O_{2} ⇌ 2 S O_{3}

, the rate of reaction was measured as

\frac{- d [O_{2}]}{d t} = 2.5 \times 10^{- 4} {mol L}^{- 1} {sec}^{- 1}

the rate of reaction expressed in terms of

S O_{3}

will be:

Q. In the formation of sulphur trioxide by the contact process,

2 S O_{2} + O_{2} ⇌ 2 S O_{3}

, the rate of reaction was measured as

- \frac{d [O_{2}]}{d t} = 3.0 \times 10^{- 4} m o l L^{- 1} s^{- 1}

.
The rate of reaction expressed in terms of

S O_{3}

will be:

In the formation of sulphur trioxide by the contact process. $2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{2} (g)$ The rate of reaction is expressed as $- \frac{d (O_{2})}{d t} = 2.5 \times 10^{- 4} m o l L^{- 1} s^{- 1}$ The rate of disappearance of $(S O_{2})$ will be:

Q. For the reaction,

2 S O_{2} + O_{2} ⇌ 2 S O_{3}

, the rate of disappearance of

O_{2}

2 \times 10^{- 4} m o l L^{- 1} s^{- 1}

. The rate of appearance of

S O_{3}

is:

Q. In the formation of sulphur trioxide by the contact process

2 S O_{2} (g) + O_{2} (g) \to 2 S O_{3} (g)

The rate of reaction is expressed as

- \frac{d (O_{2})}{d t} = 2.5 \times 10^{- 4} m o l L^{- 1} s e c^{- 1}

The rate of disappearance of

(S O_{2})

will be:

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In the reaction of formation of sulphur trioxide by contact process; 2SO2+O2⇌2SO3, the rate of reaction was measured as d[O2]dt=−2.5×10−4molL−1s−1. The rate of disappearance of [SO2] in mol.L−1s−1 will be:

The correct option is B −5.00×10−4Given that,2SO2+O2⇌2SO3Now,d[O2]dt=d[SO2]2×dt=−2.5×10−4 mol.L−1s−1d[SO2]dt=−5×10−4 mol.L−1s−1

In the reaction of formation of sulphur trioxide by contact process; $2 S O_{2} + O_{2} ⇌ 2 S O_{3}$ , the rate of reaction was measured as $\frac{d [O_{2}]}{d t} = - 2.5 \times 10^{- 4} m o l L^{- 1} s^{- 1}$ . The rate of disappearance of $[S O_{2}]$ in $m o l . L^{- 1} s^{- 1}$ will be:

The correct option is B $- 5.00 \times 10^{- 4}$
Given that,

$2 S O_{2} + O_{2} ⇌ 2 S O_{3}$

Now,

$\frac{d [O_{2}]}{d t} = \frac{d [S O_{2}]}{2 \times d t} = - 2.5 \times 10^{- 4} m o l . L^{- 1} s^{- 1}$
$\frac{d [S O_{2}]}{d t} = - 5 \times 10^{- 4} m o l . L^{- 1} s^{- 1}$