The rate of formation of NO2 for the reaction-N2O5g- 2NO2g-12O2gwas found to be 3- 10-2 mol L-1 s-1Then calculate the value of rate of disappearance of N2O5

For a given reaction, if: aA+bB→ cC+dD Overall rate r can be expressed as: r= 1a×d[A]dt= 1b×d[B]dt=+1c×d[C]dt=+1dd[D]dt where: d[A]dt=Rate of disappearance ...

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Standard VII

Chemistry

Molecularity of Reaction

The rate of f...

Question

The rate of formation of $N O_{2}$ for the reaction:
$N_{2} O_{5} (g) \to 2 N O_{2} (g) + \frac{1}{2} O_{2} (g)$
was found to be $3 \times 10^{- 2} m o l L^{- 1} s^{- 1}$
Then calculate the value of rate of disappearance of $N_{2} O_{5}$

3 \times 10^{- 2} m o l L^{- 1} s^{- 1}

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6 \times 10^{- 2} m o l L^{- 1} s^{- 1}

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1.5 \times 10^{- 2} m o l L^{- 1} s^{- 1}

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

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Solution

The correct option is C $1.5 \times 10^{- 2} m o l L^{- 1} s^{- 1}$
For a given reaction, if:
$a A + b B \to c C + d D$

Overall rate $r$ can be expressed as:

$r = \frac{- 1}{a} \times \frac{d [A]}{d t} = \frac{- 1}{b} \times \frac{d [B]}{d t} = \frac{+ 1}{c} \times \frac{d [C]}{d t} = \frac{+ 1}{d} \frac{d [D]}{d t}$
where:

$- \frac{d [A]}{d t} = Rate of disappearance of A$

$- \frac{d [B]}{d t} = Rate of disappearance of B$

$+ \frac{d [C]}{d t} = Rate of formation of C$

$+ \frac{d [D]}{d t} = Rate of formation of D$

For:
$N_{2} O_{5} (g) \to 2 N O_{2} (g) + \frac{1}{2} O_{2} (g)$

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

$Rate of formation of N O_{2} = 2 \times Rate of disappearance of N_{2} O_{5}$
$Rate of disappearance of N_{2} O_{5} = \frac{1}{2} \times 3 \times 10^{- 2} = 1.5 \times 10^{- 2} m o l L^{- 1} s^{- 1}$

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Similar questions

Q. For the reaction:

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

The value of rate of disappearance of $N_{2} O_{5}$ was found to be $6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1}$
Then choose the correct option:

Q. In a reaction,

N_{2} O_{5} \to 2 N O_{2} + \frac{1}{2} O_{2}

, the rate of disappearance of

N_{2} O_{5}

6.5 \times 10^{- 3}

m o l

L^{- 1} s^{- 1}

. Compute the rates of formation of

N O_{2}

and

O_{2}

Q. What is the ratio between the rate of decomposition of

N_{2} O_{5}

to rate of formation of

N O_{2}

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

Q. The rate constant

k

, for the reaction

N_{2} O_{5} (g) ⟶ 2 {N O}_{2} (g) + \frac{1}{2} O_{2} (g)

1.3 \times 10^{- 2} s^{- 1}

. Which equation given below describes the change of

[N_{2} O_{5}]

with time?

{[N_{2} O_{5}]}_{0}

and

{[N_{2} O_{5}]}_{t}

correspond to concentration of

N_{2} O_{5}

initially and at time

t

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:

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Molecularity of Reaction

Standard VII Chemistry

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The rate of formation of NO2 for the reaction: N2O5(g)→2NO2(g)+12O2(g) was found to be 3×10−2 molL−1s−1 Then calculate the value of rate of disappearance of N2O5

The rate of formation of $N O_{2}$ for the reaction:
$N_{2} O_{5} (g) \to 2 N O_{2} (g) + \frac{1}{2} O_{2} (g)$
was found to be $3 \times 10^{- 2} m o l L^{- 1} s^{- 1}$
Then calculate the value of rate of disappearance of $N_{2} O_{5}$