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  • <img alt="\mathrm{N}_2 \mathrm{O}_5(g) \rightarrow 2 \mathrm{NO}_2(g)+\frac{1}{2} \mathrm{O}_2(g)" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7BN%7D_2%20%5Cmathrm%7BO%7D_5%28g%2

\mathrm{N}_2 \mathrm{O}_5(g) \rightarrow 2 \mathrm{NO}_2(g)+\frac{1}{2} \mathrm{O}_2(g)
The value of rate of disappearance of  \mathrm{N}_2 \mathrm{O}_5  was found to be6.25 \times 10^{-3} \mathrm{molL}^{-1} \mathrm{~s}^{-1}  Then choose the correct option:

Option: 1

The rate of formation of  \mathrm{NO}_2  is  1.25 \times 10^{-2} \mathrm{molL}^{-1} \mathrm{~s}^{-1}


Option: 2

The rate of formation of  \mathrm{NO}_2  is  3.125 \times 10^{-3} \mathrm{molL}^{-1} \mathrm{~s}^{-1}


Option: 3

The rate of formation of  \mathrm{O}_2  is 1.25 \times 10^{-2} \mathrm{molL}^{-1} \mathrm{~s}^{-1}


Option: 4

None of the above


Answers (1)

best_answer

For a given reaction, if:
\mathrm{a A+b B \rightarrow c C+d D }
Overall rate \mathrm{r } can be expressed as:
            \mathrm{ r=\frac{-1}{a} \times \frac{d[A]}{d t}=\frac{-1}{b} \times \frac{d[B]}{d t}=\frac{+1}{c} \times \frac{d[C]}{d t}=\frac{+1 d[D]}{d d t} }
where:


\mathrm{ -\frac{d[A]}{d t}= } Rate of disappearance of A 
\mathrm{ -\frac{d[B]}{d t}= } Rate of disappearance of B
\mathrm{ -\frac{d[C]}{d t}= } Rate of disappearance of C
\mathrm{ -\frac{d[D]}{d t}= } Rate of disappearance of D

\mathrm{ \mathrm{N}_2 \mathrm{O}_5(g) \rightarrow 2 \mathrm{NO}_2(g)+\frac{1}{2} \mathrm{O}_2(g) }
           \mathrm{ r=-\frac{d\left[N_2 O_5\right]}{d t}=\frac{+1}{2} \times \frac{d\left[N O_2\right]}{d t}=+2 \times \frac{d\left[O_2\right]}{d t} }


Rate of formation of  \mathrm{\mathrm{NO}_2=2 \times}  Rate of disappearance of   \mathrm{\mathrm{N}_2 \mathrm{O}_5}
Rate of formation of

\mathrm{\mathrm{NO}_2=2 \times 6.25 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}=1.25 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}}.

Posted by

seema garhwal

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