In the formation of sulphur trioxide by the contact process- 2S O 2 - O 2 - 2S O 3- the rate of reaction was measured as - d- O 2 - dt -3-0- 10 -4 mol L -1 s -1-The rate of reaction expressed in terms of S O 3 will be-

The correct option is B 6.0× 10 ^ 4 mol L ^ 1 s ^ 1 d[ O _ 2 ] dt = 1 2 d dt [ SO _ 3 ]=3× 10 ^ 4 mol L ^ 1 s ^ 1 d ...

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Byju's Answer

Standard XII

Chemistry

Reaction Quotient

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Question

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:

3.0 \times 10^{- 4}

m o l

L^{- 1} s^{- 1}

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6.0 \times 10^{- 4}

m o l

L^{- 1} s^{- 1}

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1.5 \times 10^{- 4}

m o l

L^{- 1} s^{- 1}

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4.5 \times 10^{- 4}

m o l

L^{- 1} s^{- 1}

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Solution

The correct option is B $6.0 \times 10^{- 4}$ $m o l$ $L^{- 1} s^{- 1}$
$\frac{- d [O_{2}]}{d t} = \frac{1}{2} \frac{d}{d t} [{S O}_{3}] = 3 \times 10^{- 4} m o l L^{- 1} s^{- 1} \frac{d}{d t} [{S O}_{3}] = 6.0 \times 10^{- 4} m o l L^{- 1} s^{- 1}$

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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 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}]

m o l . L^{- 1} s^{- 1}

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. 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:

Q. How long does it take for reactant concentration to decrease from

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

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

in a zero order reaction.

Rate constant of the reaction, k = 5 \times 10^{- 8} m o l L^{- 1} s^{- 1}

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In the formation of sulphur trioxide by the contact process, 2SO2+O2⇌2SO3, the rate of reaction was measured as −d[O2]dt=3.0×10−4 mol L−1s−1.The rate of reaction expressed in terms of SO3 will be:

The correct option is B 6.0×10−4 mol L−1s−1−d[O2]dt=12ddt[SO3]=3×10−4molL−1s−1ddt[SO3]=6.0×10−4molL−1s−1

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:

The correct option is B $6.0 \times 10^{- 4}$ $m o l$ $L^{- 1} s^{- 1}$
$\frac{- d [O_{2}]}{d t} = \frac{1}{2} \frac{d}{d t} [{S O}_{3}] = 3 \times 10^{- 4} m o l L^{- 1} s^{- 1} \frac{d}{d t} [{S O}_{3}] = 6.0 \times 10^{- 4} m o l L^{- 1} s^{- 1}$