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- - Chemistry Q-A

Step 1 Given data:Given reaction 2N_2O_5(g)→ 4NO_2(g) + O_2(g)Rate of formation of NO_2(g)=2.8×10^ 3Ms^ 1Step 2: Applying the formula: ⇒ 1/2d/dt[N_2O_5]=1/4d/ ...

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

Byju's Answer

Standard XII

Chemistry

Reaction Quotient

For The React...

Question

For the reaction $\underset{Dinitrogen pentoxide}{\underset{⏟}{2 N_{2} O_{5} (g)}} \to \underset{Nitrogen dioxide}{\underset{⏟}{4 {NO}_{2}}} (g) + \underset{Oxygen}{\underset{⏟}{O_{2} (g)}}$ . The rate of formation of ${NO}_{2} (g)$ is $2.8 \times 10^{- 3} {Ms}^{- 1}$ . Calculate the rate of disappearance of $N_{2} O_{5} (g)$ .

Open in App

Solution

Step 1 Given data:
Given reaction $2 N_{2} O_{5} (g) \to 4 {NO}_{2} (g) + O_{2} (g)$
Rate of formation of ${NO}_{2} (g) = 2.8 \times 10^{- 3} {Ms}^{- 1}$
Step 2: Applying the formula:
$\Rightarrow - \frac{1}{2} \frac{d}{dt} [N_{2} O_{5}] = \frac{1}{4} \frac{d}{dt} [{NO}_{2}] \Rightarrow - \frac{d}{dt} [N_{2} O_{5}] = 2 \times \frac{1}{4} \frac{d}{dt} [{NO}_{2}] \Rightarrow - \frac{d}{dt} [N_{2} O_{5}] = \frac{1}{2} \frac{d}{dt} [{NO}_{2}] \Rightarrow - \frac{d}{dt} [N_{2} O_{5}] = \frac{1}{2} \times 2.8 \times 10^{- 3} {Ms}^{- 1} \Rightarrow - \frac{d}{dt} [N_{2} O_{5}] = 1.4 \times 10^{- 3} {Ms}^{- 1} \Rightarrow 1.4 \times 10^{- 3} {Ms}^{- 1}$
Therefore, the rate of disappearance of $N_{2} O_{5} (g)$ is $1.4 x 10^{- 3} {Ms}^{- 1}$ .

Suggest Corrections

Similar questions

C H_{3} C O O C_{2} H_{5} (a q) + N a O H (a q) ⟶ C H_{3} C O O N a (a q) + C_{2} H_{5} O H (a q)

Which one of the following statements is correct for the reaction?

Q. For the reaction,

N_{2} O_{4} (g) {⇌ K_{2}}^{K_{1}} 2 N O_{2} (g)

, the rate of disappearance of

N O_{2}

will be :

Q. Halogenation is a substitution reaction, where halogen replaces one or more hydrogens of hydrocarbon.
Chlorine free radical make

1^{\circ}, 2^{\circ}, 3^{\circ}

radicals with almost equal ease, whereas bromine free radicals have a clear preference for the formation of tertiary free radicals. So , bromine is less reactive, and more selective whereas chlorine is less selective and more effective.
The relative rate of abstraction of hydrogen by Br is

3^{\circ} (1600) > 2^{\circ} (82) > 1^{\circ} (1)

The relative rate of abstraction of hydrogen by Cl is

3^{\circ} (5) > 2^{\circ} (3.8) > 1^{\circ} (1)

F. What would be the product ratio x/y in the chlorination of propane if all the hydrogen were abstracted at equal rate ?

C H_{3} - C H_{2} - C H_{3} C l_{2} - - \to h v C H_{3} - C H_{2} - C (x) H_{2} - C l + C H_{3} - C | C l (y) H - C H_{3}

Q. 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)

C H_{3} - C H_{3} | C | B r - C H_{3}, C H_{3} - C | B r - C H_{3}, C H_{3} - C H - B r

Compare rate of

E_{2}

reaction :

Join BYJU'S Learning Program

For the reaction2N2O5(g)⏟Dinitrogenpentoxide→4NO2⏟Nitrogendioxide(g)+O2(g)⏟Oxygen. The rate of formation of NO2(g)is 2.8×10-3Ms-1. Calculate the rate of disappearance of N2O5(g).