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?
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 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.
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.
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.
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.
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 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|