Following data are obtained for reaction :
N2O5 → 2NO2 + 1/2O2
|[N2O5]/mol L–1||1.6 × 10-2||0.8 × 10–2||0.4 × 10–2|
1) Show that it follows first order reaction.
2) Calculate the half-life.
(Given log 2 = 0.3010, log 4 = 0.6021)
The rate constant for a first order reaction is 60 s−1. How much time will it take to reduce the initial concentration of the reactant to its 1/16th value?
For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data are obtained.
|t (sec)||P(mm of Hg)|
Calculate the rate constant.
The following data were obtained during the first order thermal decomposition of SO2Cl2 at a constant volume :SO2Cl2 (g) → SO2 (g) + Cl2 (g)
Calculate the rate of the reaction when total pressure is 0.65 atm.
A reaction is first order in A and second order in B. How is the rate affected when the concentrations of both A and B are doubled?
A reaction is first order in A and second order in B. How is the rate affected on increasing the concentration of B three times?
The time required for 10% completion of a first order reaction at 298 K is equal to that required for its 25% completion at 308 K. If the value of A is 4 × 1010 s−1. Calculate k at 318 K and Ea.
In a pseudo first order hydrolysis of ester in water, the following results were obtained:
(i) Calculate the average rate of reaction between the time interval 30 to 60 seconds.
(ii) Calculate the pseudo first order rate constant for the hydrolysis of ester.
A first order reaction takes 20 minutes for 25% decomposition. Calculate the time when 75% of the reaction will be completed.
(Given : log = 2 = 0·3010, log 3 = 0·4771, log 4 = 0·6021)
The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
|Experiment||A/ mol L−1||B/ mol L−1||Initial rate/mol L−1 min−1|
|I||0.1||0.1||2.0 × 10−2|
|II||--||0.2||4.0 × 10−2|
|IV||--||0.2||2.0 × 10−2|