Home
Class 12
CHEMISTRY
For the reaction 2 N2O5(g) to 4 NO2(g) ...

For the reaction `2 N_2O_5(g) to 4 NO_2(g) + O_2 (g)` in liquid bromine, `N_2 O_5` disappears at a rate of 0.02 moles `dm^(-3) sec^(-1)` At what rate `NO_2` and `O_2` are formed? What would be the rate of reaction?

Text Solution

Verified by Experts

Given : `(d[N_2O_5])/(dt) = 0.02 1/4 (d[NO_2])/(dt)`
`= (d[O_2])/(dt)`
Rate of reaction ` = -1/2 (d[N_2O_5])/(dt)`
`= 1/2 (d[N_2O_5])/(dt)`
Rate of formation of `O_2 = (d[O_2])/(dt) = 1/2 xx 0.02`
` = 1/2 - (d[N_2O_5])/(dt) = 1/2 xx 0.02 ` moles `dm^(-3) sec^(-1) = 0.01 ` moles `dm^(-3) sec^(-1)`
Rate of formation of `NO_2 = (d[NO_5])/(dt)`
`= 4/2- (d[N_2O_5])/(dt)`
`= 2 xx ` moles `dm^3 sec^(-1)`
= 0.04 moles `dm^3 sec^(-1)`
Promotional Banner

Similar Questions

Explore conceptually related problems

Write the expression for: 2 N_2O(g)rarr 4 NO_2(g) + O_2(g) ?

At a particular moment during the reaction 2N_(2) O_(5) to 4NO_(2) +O_(2) in liquid bromine N_(2) O_(5) disappears at a rate of 0.03 M/s . What is the rate of NO_(2) formation ?

The elementary reaction O_3(g) + O(g) rarr 2 O_2(g) is

Consider the reaction 2N_(2) O_(5(g) ) to 4NO_(2(g)) +O_(2(g)) in liquid bromine If -(d[N_(2)O_(5) ])/(dt)=0.02 M s^(-1) then NO_(2) is formed at _______.

In the reaction 2N_2O_(5(g)) rarr 4NO_(2(g)) + O_2 at a certain time. The rate of formation of NO_2 is 0.08 Ms^(-1) . Find the rate of consumption of N_2O_5 , rate of formation of O_2 and the rate of the reaction.

The order of the reaction 2NO_(g)+O_(2(g))rarr 2NO_(2(g)) having Rate = k[NO_2]^2[O_2] is