EASY
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Identify a concentration verses time graph for a second order reaction with single reactant.

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Important Questions on Chemical Kinetics (AHL)

MEDIUM

For a reaction, consider the plot of lnk versus 1/T given in the figure. If the rate constant of this reaction at 400K is 10-5s-1 , then the rate constant at 500K is:

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EASY
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?
HARD

For an elementary chemical reaction, A2 k-1k12A , the expression for dAdt is:

EASY
The rate constant of the reaction AB is 0.6×10-3 mole per liter per second. If the initial concentration of A is 5 M, then the concentration of B after 20 minutes is:
HARD
According to the Arrhenius equation,
HARD
Consider the following reversible reaction:

A g+B gAB g

The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in  mol-1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of G  (in J mol-1) for the reaction at 300 K is ____.

(Given; ln2= 0.7,  = 2500 J mol-1 at 300 K and G is the Gibbs energy)
MEDIUM
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?
EASY
For the equilibrium, AgBg, H is -40 kJ/mol . If the ratio of the activation energies of the forward Ef and reverse Eb reactions is 23 then:
EASY
The addition of a catalyst during a chemical reaction alters which of the following quantities?
MEDIUM
The rate of a first-order reaction is 0.04 mol l-1s-1 at 10 second and 0.03 mol l-1s-1 at 20 seconds after initiation of the reaction. The half-life period of the reaction is:
EASY
The rate of a reaction doubles when its temperature changes from 300K to 310K. Activation energy of such a reaction will be:

R=8.314 JK-1mol-1 and log 2=0.301
EASY

For the reaction,

A+BP=-d[A]dt=-d[B]dt=k[A][B] and

kt=1[A]0-[B]0ln[A][B]0[B][A]0 when, [A]0[B]0
If, [A]0=[B]0 then the integrated rate law will he

HARD
The reaction 2N2O5g4NO2g+O2(g) follows first order kinetics. The pressure of a vessel containing only N2O5 was found to increase from 50 mm Hg to 87.5 mm Hg in 30 min. The pressure exerted by the gases after 60 min. Will be (Assume temperature remains constant) :
HARD
For a first order reaction A(g)  2B(g) + C(g) at constant volume and 300 K, the total pressure at the beginning (t = 0) and at time are  p0 and pt, respectively. Initially, only A is present with concentration  A0, and  t13  is the time required for the partial pressure of A to reach 1/3rd of its initial value. The correct option(s) is (are)
(Assume that all these gases behave as ideal gases)
EASY
A+2BC , the rate equation for the reaction is given as

Rate =k[A][B]

If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself?
MEDIUM
A reaction has an activation energy of 209 kJ mol-1 . The rate increases 10 -fold when the temperature is increased from 27oC to XoC . The temperature X is closest to

[Gas constant, R=8.314 J mol-1K-1 ]
MEDIUM
For the non-stoichiometry reaction,  2 A + B C + D , the following kinetic data were obtained in three separate experiments, all at 298 K.
Initial Concentration (A) Initial Concentration (B) Initial rate of formation of C mol L - S -  
0.1 M 0.1 M 1.2 × 1 0 - 3
0.1 M 0.2 M 1.2 × 1 0 - 3
0.2 M 0.1 M 2.4 × 1 0 - 3

The rate law for the formation of C is 
HARD

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 )

(I) 

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(II) 

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MEDIUM
For a second order reaction, (2A Product) 1A vs t is represented as
EASY
The ratio of the half-life time t1/2, to the three quarter life-time, t3/4, for a reaction that is sècond order