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The following results were obtained during kinetic studies of the reaction.

2A+B product
 
Experiment A in mol L-1 B  in mol L-1 Initial rate of reaction in mol L-1 min -1
I 0.10 0.20 6.93×10-3
II 0.10 0.25 6.93×10-3
III 0.20 0.30 1.386×10-2

The time (in minutes) required to consume half of A is

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Important Questions on Chemical Kinetics

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For the reaction, 2A+B products, when the concentration of A and B both were doubled, the rate of the reaction increased from 0.3 mol L-1s-1 to 2.4 mol L-1s-1.  When the concentration of A alone is doubled, the rate increased from 0.3 mol L-1s-1 to 0.6 mol L-1s-1.

Which one of the following statements is correct?
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Consider the given plots for a reaction obeying Arrhenius equation 0°C<T<300°C(k and Ea are rate constant and activation energy, respectively)

IQuestion Image 

IIQuestion Image

Choose the correct option:

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For an elementary chemical reaction,

A2k-1k12A the expression for d[A]dt

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If a reaction follows the Arrhenius equation, the plot lnk vs 1RT gives straight line with a gradient -y unit. The energy required to activate the reactant is:
 
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The reaction 2XB is a zeroth order reaction. If the initial concentration of X is 0.2 M, the half-life is 6 h. When the initial concentration of X is 0.5 M, the time required to reach its final concentration of 0.2 M will be:
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Decomposition of X exhibits a rate constant of 0.05μg/year. How many years are required for the decomposition of 5μg of X into 2.5μg?
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For a reaction, consider the plot of In k versus 1/T given in the figure. If the rate constant of this reaction at 400 K is 10-5 s-1, then the rate constant at 500 K is :

Question Image

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In the formation of sulphur trioxide by the contact process 2SO2(g)+O2(g)2SO3(g). The rate of reaction is expressed as -dO2dt=2.5×10-4molL-1sec-1. The rate of disappearance of SO2 will be:-