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For the first order reaction 2N2O5 (g) r...

For the first order reaction `2N_2O_5 (g) rarr 4 NO_2(g)+ O_2(g)` which is incorrect:-

A

the concentration of the reactant decreases exponentially with time.

B

the half-life of the reaction decreases with increasing temperature.

C

the half-life of the reaction depends on the initial concentration of the reactant.

D

the reaction proceeds to 99.6% completion in eight half-life duration.

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The initial concentration of N_2O_5 in the following first order reaction N_2O_5(g) rarr 2 NO_2(g) + 1/2O_2 (g) was 1.24 x 10^(-2) mol L^(-1) Calculated the rate constant of the reaction at 318 K.

Nitrogen pentoxide decomposes according to equation : 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) This first order reaction was allowed to proceed at 40^@ C and the data below were collected : What will be the concentration of N_2O_5 after 100 minutes ?

Nitrogen pentoxide decomposes according to equation : 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) This first order reaction was allowed to proceed at 40^@ C and the data below were collected : Calculate the rate constant. Include units with your answer.

The decomposition of N_2O_5 according to the equation, 2N_2O_5(g) harr 4NO_2(g) + O_2(g) is a first order reaction. After 30 min from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm of Hg and on complete decomposition, the total pressure is 584.5 mm of Hg. Calculate the rate constant of the reaction.

The decomposition of N_2O_5 in CC1_4 at 318K has been studied by monitoring the concentration of N_2O_5 in the solution. Initially the concentration of N_2O_5 is 2.33 mol L^(-1) and after 184 minutes, it is reduced to 2.08 mol L^(-1) . The reaction takes place according to the equation 2 N_2O_5 (g) rarr 4 NO_2 (g) + O_2 (g) 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 period?

The integrated rate equations can be fitted with kinetic data to determine the order of a reaction. The integrated rate equations for zero, first and second order reactions are : Zero order : [Al =-kt+ [A]_0 First order : log [A] = -(kt)/2.303 + log [A]_0 Second order : 1/([A])=kt+1/[A]_0 These equations can also be used to calculate the halt life periods of different reactions, which give the time during which the concentration of a reactant is reduced to half of its initial concentration, i.e, at time t_(1//2), [A] = [A]_0//2 Answer the following (1 to 5) question : The decomposition of nitrogen pentoxide : 2N_2O_5(g) rarr 4NO_2(g) + O_2(g) is a first order reaction. The plot of log [N_2O_5] vs time (min) has slope = - 0.01389. The rate constant k is

For the reaction N_2O_5(g)rarr 2NO_2(g) + 1/2 O_2 (g) the value of rate of disappearance of N_2O_5 is given as 6.25 xx 10^-3 mol L^-1 s^-1 . The rate of formation of NO_2 and O_2 is given respectively as :

The molecularity of the reaction 2NO+O_2 rarr 2 NO_2 is,

For the reactions : C(s) + O_(2) (g) to CO_(2) (g)

MODERN PUBLICATION-CHEMICAL KINETICS-EXERCISE
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  2. Fill in the blanks- is an mixture which is used as domestic fuel.

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  3. For the first order reaction 2N2O5 (g) rarr 4 NO2(g)+ O2(g) which is i...

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  4. Consider the following reaction for 2NO2(g) + F2(g) rarr 2NO2F(g). The...

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  5. Arrhenius equation is

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  6. The integrated rate equations can be fitted with kinetic data to deter...

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  7. The integrated rate equations can be fitted with kinetic data to deter...

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  8. The integrated rate equations can be fitted with kinetic data to deter...

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  9. The integrated rate equations can be fitted with kinetic data to deter...

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  10. For a zero order reaction, linear plot was obtained for [A] vs t. The ...

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  11. According to collision theory of chemical reactions, rate of a reactio...

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  12. For a first order reaction, the plot of log K versus 1/T gives straigh...

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  13. The pre-expotential factor in Arrhenius equation of a second order rea...

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  14. At 27^@C in the presence of a catalyst, the activation energy of a rea...

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  15. The rate of a chemical reaction becomes double for every 10^@C rise in...

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