For the reaction- 2 SO 2- O 2- 2 SO 3- the rate of disappearance of O 2 is 2 - 10-4 molL -1 s -1- The rate of appearance of SO 3 is-A- 2 - 10-4 molL -1 s -1B- 4 - 10-4 molL -1 s -1C- 1 - 10-1 molL -1 s -1D- 6 - 10-4 molL -1 s -1

For the reaction, $N_{2} O_{5} (g) \to N O_{2} (g) + \frac{1}{2} O_{2} (g)$ The value of rate of disappearance of $N_{2} O_{5}$ is given as $6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1} .$ The rate of formation of $N O_{2}$ and $O_{2}$ is given respectively as:

Q. For the reaction,

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

rate and rate constant are

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

and

3.4 \times 10^{- 5} s^{- 1}

respectively. The concentration of

N_{2} O_{5}

in mol

L^{- 1}

will be:

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For the reaction, 2SO2+O2⇌2SO3, the rate of disappearance of O2 is 2×10−4 molL−1s−1. The rate of appearance of SO3 is:

The correct option is B 4×10−4 molL−1s−1For the given reaction, rate can be expressed as: (rate) r =r(SO3)2=−r(O2)1 r(SO3)= 2 × r(O2)= 2 × ( 2 ×10−4) rate = 4 ×10−4 molL−1s−1

For the reaction, $2 S O_{2} + O_{2} ⇌ 2 S O_{3}$ , the rate of disappearance of $O_{2}$ is $2 \times 10^{- 4} m o l L^{- 1} s^{- 1}$ . The rate of appearance of $S O_{3}$ is:

The correct option is B $4 \times 10^{- 4} mol L^{- 1} s^{- 1}$
For the given reaction, rate can be expressed as:
(rate) r = $\frac{r (S O_{3})}{2}$ = $- \frac{r (O_{2})}{1}$
r( $S O_{3}$ )= 2 $\times$ r( $O_{2}$ )= 2 $\times$ ( 2 $\times 10^{- 4})$
rate = 4 $\times 10^{- 4} m o l L^{- 1} s^{- 1}$