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While studying the decompoistion of gase...

While studying the decompoistion of gaseous `N_(2)O_(5)`, it is observed that a plot of logarithm of its partial pressure versus time is linear. What kinetic parameters can be obtained form this observation?

A

rate constant

B

initial concentration of `N_2O_5`

C

both

D

energy of activation

Text Solution

Verified by Experts

The linear graph plotted between log `P_(N_2O_5)` and t shows that it is a first order reaction.
From its slope, k can be evaluated and from the intercept, the `P_(N_2O_5)^0`
(Initial pressure of `N_2O_5`) can be determined.
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A : The decomposition of gaseous N_2O_5 follows first order kinetics. R : The plot of log of its partial pressure versus time is linear with slope , -k/(2.303) and having intercept equal to log P.

In the decompoistion of N_(2)O_(5) , the plot between the reciprocal of concentration of the reactant and the time was found to be linear as shown in figure below. Determine the order of reaction.

The gas phase decomposition of N_(2)O_(5)" to "NO_(2) and O_(2) is monitored by measurement of total pressure. The following data are obtained. Find the average rate of disappearance of N_(2)O_(5) for the time interval between each interval and for the total time interval. [Hint : Integrated rate law is NOT to be used]

Reaction rate : At some time, we observe that the reaction 2N_(2)O_(5)(g)rarr 4NO_(2)(g)+O_(2)(g) is forming NO_(2) at the rate of 0.0072 mol L^(-1)s^(-1) . (i) What is the rate of reaction at this time ? (ii) What is the rate of formation of O_(2) at this time ? (iii) What is the rate of consumption of N_(2)O_(5) at this time ? Strategy : For expressing the rate of such reaction where stoichiometric coefficents of reactants or products are not equal to one, rate of any of the products is divided by their respective stoichiometric coefficients. Use the mole ratios from the balanced equation to determine the rates of change of other products and reactants.

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The decompoistion of N_(2)O_(5) in C CI_(4) solution at 318 K has been studied by monitoring the concentration of N_(2)O_(5) in the solution. Initially, the concentration of N_(2)O_(5) is 2.33 M and after 184 min , it is reduced to 2.08 M . The reaction takes place according to the equation: 2N_(2)O_(5) rarr 4NO_(2) + O_(2) Calculate the average rate of this reaction in terms of hours, minutes, and seconds. What is the rate of Production of NO_(2) during this periof?

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