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−1 s−1. The rate of reaction expressed in terms of SO3 will be

−d[O2]dt=+12d[SO3]dt3×10−4=12d[SO3]dtd[SO3]dt=6×10−4 M/sec

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−1 s−1. The rate of reaction expressed in terms of SO3 will be

−d[O2]dt=+12d[SO3]dt3×10−4=12d[SO3]dtd[SO3]dt=6×10−4 M/sec

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In the formation of sulphur trioxide by the contact process, $2 {SO}_{2} + O_{2} ⇌ 2 {SO}_{3}$ , the rate of reaction was measured as $\frac{d [O_{2}]}{dt} = 3 .0 \times 10^{- 4} mol L^{- 1} s^{- 1}$ .
The rate of reaction expressed in terms of ${SO}_{3}$ will be

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$3 .0 \times 10^{- 4} mol L^{- 1} s^{- 1}$

$6 .0 \times 10^{- 4} mol L^{- 1} s^{- 1}$

$1 .5 \times 10^{- 4} mol L^{- 1} s^{- 1}$

$4 .5 \times 10^{- 4} mol L^{- 1} s^{- 1}$

answer is B.

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$\begin{array}{l} - \frac{d [O_{2}]}{dt} = + \frac{1}{2} \frac{d [{SO}_{3}]}{dt} \\ 3 \times 10^{- 4} = \frac{1}{2} \frac{d [{SO}_{3}]}{dt} \\ \frac{d [{SO}_{3}]}{dt} = 6 \times 10^{- 4} M/sec \end{array}$

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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−1 s−1. The rate of reaction expressed in terms of SO3 will be

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In the formation of sulphur trioxide by the contact process, $2 {SO}_{2} + O_{2} ⇌ 2 {SO}_{3}$ , the rate of reaction was measured as $\frac{d [O_{2}]}{dt} = 3 .0 \times 10^{- 4} mol L^{- 1} s^{- 1}$ .
The rate of reaction expressed in terms of ${SO}_{3}$ will be