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The reaction 2N(2)O(5)((g)rarr4NO(2)(g...

The reaction `2N_(2)O_(5)((g)rarr4NO_(2)(g)+O_(2)(g)` provides a linear plot when In `P_(n_(2)O_(5)` is plotted against t with a negative slope. The decomposition of `N_(2)O_(5)` follows

A

zero order kinetics

B

first order kinetics

C

third order kinetics

D

second order kinetics

Text Solution

Verified by Experts

The correct Answer is:
B
For a first order reaction in `[A]_(0)-In [A]_(t)=kt` ie In `[A]_(t)=In[A]_(0)-kt`
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The decomposition of N_(2)O_(5) according to the equation, 2N_(2)O_(5) (g) rarr 4NO_(2) (g) + O_(2) (g) is a first order reaction, After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm Hg and on completion, the total pressure is 584.5 mm Hg. Calculate the rate constant of the reaction.

Consider the reaction 4NO_(2(g)) + O _(2 (g)) to 2 N _(2 ) O _(5(g)) , Delta H =-111 kJ If N _(2 ) O _(5 (s)) is formed in the above reaction Delta H will be (Given Delta H for sublimation of N_(2) O_(5) is 54 kJ)

The rate equation for 2N_(2)O_(5) rarr 4NO_(2) + O_(2) is r = (6.3xx10^(-4)s^(-1))[N_(2)O_(5)] . The initial rate of decomposition of 0.1 MN_(2) O_(5) will be

In the process 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) at t = 10, rate of reaction w.r.t. N_(2)O_(5), NO_(2) & O_(2) respectively are:

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