For the reaction; 2N2O5g→4NO2g+O2gif the concentration of NO2 increases by  5.2×10-3M 100 seconds then the rate of the reaction is

# For the reaction; $2{\mathrm{N}}_{2}{\mathrm{O}}_{5\left(\mathrm{g}\right)}\to 4{\mathrm{NO}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}$if the concentration of ${\mathrm{NO}}_{2}$ increases by

1. A

2. B

3. C

4. D

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### Solution:

$2{\mathrm{N}}_{2}{\mathrm{O}}_{5\left(\mathrm{g}\right)}\to 4{\mathrm{NO}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}$

Rate of appearance of ${\mathrm{NO}}_{2}$ is $=\frac{5.2×{10}^{-3}}{100}$

rate  of reaction $=\frac{1}{4}\frac{\mathrm{d}\left[{\mathrm{NO}}_{2}\right]}{\mathrm{dt}}$

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