For the reaction 2N2O5g- 4NO2g-O2g- the rate of formation of NO2g is 2-8- 10-3M s-1- Calculate the rate of disappearance of N2O5g-

For the reaction 2N_2O_5(g)→ 4NO_2(g)+O_2(g) , the rate of formation of NO_2 (g) is 2.8× 10^ 3M s^ 1 . ddt[NO_2]=2.8× 10^ 3M s^ 1 The rate of ...

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Byju's Answer

Standard XII

Chemistry

Elementary and Complex Reactions

For the react...

Question

For the reaction $2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)$ , the rate of formation of $N O_{2}$ (g) is $2.8 \times 10^{- 3} M s^{- 1}$ . Calculate the rate of disappearance of $N_{2} O_{5} (g)$ .

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Solution

For the reaction $2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)$ , the rate of formation of $N O_{2}$ (g) is $2.8 \times 10^{- 3} M s^{- 1}$ .
$\frac{d}{d t} [N O_{2}] = 2.8 \times 10^{- 3} M s^{- 1}$
The rate of disappearance of $N_{2} O_{5} (g)$ .
$- \frac{1}{2} \frac{d}{d t} [N_{2} O_{5}] = \frac{1}{4} \frac{d}{d t} [N O_{2}]$

$- \frac{d}{d t} [N_{2} O_{5}] = 2 \times \frac{1}{4} \frac{d}{d t} [N O_{2}]$

$- \frac{d}{d t} [N_{2} O_{5}] = \frac{1}{2} \frac{d}{d t} [N O_{2}]$

$- \frac{d}{d t} [N_{2} O_{5}] = \frac{1}{2} \times 2.8 \times 10^{- 3} M s^{- 1}$

$- \frac{d}{d t} [N_{2} O_{5}] = 1.4 \times 10^{- 3} M s^{- 1}$

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Similar questions

Q. For the reaction

2 N_{2} O_{5} (g) ⟶ 4 N O_{2} (g) + O_{2} (g),

the rate of formation of

N O_{2} (g)

2.8 \times 10^{- 3} m o l s^{- 1} .

Calculate the rate of disapperance of

N_{2} O_{5} (g) .

Q. For the reaction

2 N_{2} O_{5} (g) ⟶ 4 N O_{2} (g) + O_{2} (g),

the rate of formation of

N O_{2} (g)

2.8 \times 10^{- 3} m o l s^{- 1} .

Calculate the rate of disapperance of

N_{2} O_{5} (g) .

Q. For a first order reaction involving decomposition of

N_{2} O_{5}

the following information is available

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)

rate

= k [N_{2} O_{5}]

N_{2} O_{5} (g) \to 2 N O_{2} (g) + 1 / 2 O_{2} (g)

rate

= k^{'} [N_{2} O_{5}]

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. Derive an expression for the Rate (k) of reaction :

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)

With the help of following mechanism:

N_{2} O_{5}_{a} N O_{2} + N O_{3}

N O_{3} + N O_{2}_{- a} N_{2} O_{5}

N O_{2} + N O_{3}_{b} N O_{2} + O_{2} + N O

N O + N O_{3}_{c} 2 N O_{2}

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For the reaction 2N2O5(g)→4NO2(g)+O2(g), the rate of formation of NO2(g) is 2.8×10−3Ms−1. Calculate the rate of disappearance of N2O5(g).

For the reaction $2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)$ , the rate of formation of $N O_{2}$ (g) is $2.8 \times 10^{- 3} M s^{- 1}$ . Calculate the rate of disappearance of $N_{2} O_{5} (g)$ .