Home
Class 12
CHEMISTRY
Gaseous N(2)O(5) decomposes according to...

Gaseous `N_(2)O_(5)` decomposes according to the following equation:
`N_(2)O_(5)(g) rarr 2NO_(2)(g) + (1)/(2)O_(2)(g)`
The experimental rate law is `-Delta [N_(2)O_(5)]//Delta t = k[N_(2)O_(5)]`. At a certain temerature the rate constant is `k = 5.0 xx 10^(-4) sec^(-1)`. In how seconds will the concentration of `N_(2)O_(5)` decrease to one-tenth of its initial value ?

Promotional Banner

Similar Questions

Explore conceptually related problems

Discuss the rate of the reaction 2N_(2)O_(5(g)) rarr 4NO_(2(g))+O_(2(g))

Discuss the rate of the reaction 2N_(2)O_(5(g)) rarr 4NO_(2(g))+O_(2(g))

Discuss the rate of the reaction 2N_(2)O_(5(g)) rarr 4NO_(2(g))+O_(2(g))

Discuss the rate of the reaction 2N_(2)O_(5(g)) rarr 4NO_(2(g))+O_(2(g))

For the reaction 2N_(2) O_(5) (g) overset(k)rarr 4NO_(2) (g) + O_(2) (g) having rate law. Rate = k [N_(2)O_(5)]=R_(1) Select correct statement.

For the reaction 2N_(2)O_(5) rarr 4NO_(2)+O_(2) rate of reaction and rate constant are 1.02 xx 10^(-4) and 3.4 xx 10^(-5) sec^(-1) respectively. The concentration of N_(2)O_(5) at that time will be

For the reaction, 2N_(2)O_(5)to4NO_(2)+O_(2) rate and rate constant are 1.02xx10^(-4) M sec^(-1) and 3.4xx10^(-5)sec^(-1) respectively, the concentration of N_(2)O_(5) , at that time will be

For the reaction, 2N_(2)O_(5)to4NO_(2)+O_(2) rate and rate constant are 1.02xx10^(-4) M sec^(-1) and 3.4xx10^(-5)sec^(-1) respectively, the concentration of N_(2)O_(5) , at that time will be

For the reaction 2N_(2)O_(5)to4NO_(2)+O_(2) , rate and rate constant are 1.02xx10^(-4)M"sec"^(-1) and 3.4xx10^(-5)"sec"^(-1) respectively then concentration of N_(2)O_(5) at that time will be (in moles /lit)