For the reaction- N 2 O 5 g - NO 2 g -1-2 O 2 g The value of rate of disappearance of N 2 O 5 is given as 6-25 - 10-3 molL -1 s -1- The rate offormation of NO 2 and O 2 is given respectively as-A- 1-25 - 10-2 molL -1 s -1 and 3-125 - 10-3 molL -1 s -1B- 6-25 - 10-3 molL -1 s -1 and 3-125 - 10-3 mol L -1 s -1C- 1-25 - 10- 2 molL -1 s -1 and 6-25 - 10-3 molL -1 s -1D- 6-25 - 10-3 molL -1 s -1 and 6-25 - 10-3 molL -1 s -1

The correct option is A 1.25 × 10^ 2 mol L^ 1 s^ 1 and 3.125 × 10^ 3 mol L^ 1 s^ 1 Rate of disappearance of reactant = rate of appearance of product Or 1/Sto ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard VII

Chemistry

Rate of Reaction

For the react...

Question

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:

$6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1} a n d 6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$1.25 \times 10^{- 2} m o l L^{- 1} s^{- 1} a n d 3.125 \times 10^{- 3} m o l L^{- 1} s^{- 1}$

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

$6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1} a n d 3.125 \times 10^{- 3} m o l L^{- 1} s^{- 1}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

$1.25 \times 10^{-} 2 m o l L^{- 1} s^{- 1} a n d 6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1}$

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B
$1.25 \times 10^{- 2} m o l L^{- 1} s^{- 1} a n d 3.125 \times 10^{- 3} m o l L^{- 1} s^{- 1}$

Rate of disappearance of reactant = rate of appearance of product
Or - $\frac{1}{S t o i c h i o m e t r i c c o e f f i c i e n t o f r e a c t a n t} \frac{d [r e a c t a n t]}{d t}$
$+ \frac{1}{S t o i c h i o m e t r i c c o e f f i c i e n t o f p r o d u c t} \frac{d [p r o d u c t]}{d t}$
For the reaction,
$N_{2} O_{5} (g) \to 2 N O_{2} (g) + \frac{1}{2} O_{2} (g) - \frac{d [N_{2} O_{5}]}{d t} = + \frac{1}{2} \frac{d [N O_{2}]}{d t} = + \frac{2 d [O_{2}]}{d t}$
$∴ \frac{d [N O_{2}]}{d t} = - 2 \frac{d [N_{2} O_{5}]}{d t} = 2 \times 6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1} = 12.5 \times 10^{(} - 3) m o l L^{- 1} s^{- 1}$
$= 1.25 \times 10^{- 2} m o l L^{- 1} s^{- 1} \frac{d [O_{2}]}{d t} = - \frac{d [N_{2} O_{5}]}{d t} \times \frac{1}{2} = \frac{6.25 \times 10^{- 3} m o l L^{- 1} s^{- 1}}{2} = 3.125 \times 10^{- 3} m o l L^{- 1} s^{- 1}$

Suggest Corrections

Similar questions

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:

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. For the reaction 2A + B + C

\to A_{2} B

+ C the rate law is found to be Rate =k[A][B]

^{2}

with

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

The initial rate of reaction with

[A] = 0.1 m o l L^{- 1}, [B] = 0.2 m o l L^{- 1} a n d [C] = 0.8 m o l L^{- 1}

Q. For the reaction,

2 S O_{2} + O_{2} ⇌ 2 S O_{3}

, the rate of disappearance of

O_{2}

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

. The rate of appearance of

S O_{3}

is:

At 27°C and 37°C the rates of a reaction are given as 1.6*10^-2 mol L^-1s^-1 and 3.2*10^-2 mol L^-1s^-1.Calculate the energy of activation for the give reaction.

Join BYJU'S Learning Program

For the reaction, N2O5(g)→NO2(g)+12O2(g) The value of rate of disappearance of N2O5 is given as 6.25×10−3molL−1s−1. The rate of formation of NO2 and O2 is given respectively as:

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: