Chemical Kinetics and Nuclear Chemistry

During the nuclear explosion, one of the products is 90Sr with half life of 6.93 years. If 1 \(\mu\) g of 90Sr was absorbed in the bones of newly born baby in placed of Ca, how much time, in years, is required to reduce much time, in year,...

For the reaction 2H2(g) + 2NO(g) \(\to\) N2(g) + 2H2O(g) the observed rate expression is, rate = Kf[NO]2[H2]. The rate expression for the reverse reaction is :

Consider the following reactions
A \(\to\) P1 ; B \(\to\) P2 ; C \(\to\) P3 ; D \(\to\) P4,
The order of the above reactions are a, b, c,
and d, respectively. The following graph is
obtained when log[rate] vs. log[conc.] are
plotted...

The rate of a reaction decreased by 3.555
times when the temperature was changed
from 40oC to 30oC. The activation energy
(in kJ mol–1) of the reaction is _______.
Take;
R = 8.314 J mol–1 K–1 ln 3.555 = 1.268

A flask contains a mixture of compounds A and
B. Both compounds decompose by first-order
kinetics. The half-lives for A and B are 300 s
and 180 s, respectively. If the concentrations
of A and B are equal initially, the time required
for the...

The rate constant (k) of a reaction is measured at differenct temperatures (T), and the data are
plotted in the given figure. The activation energy of the reaction in kJ mol–1 is :
(R is gas constant)

If 75% of a first order reaction was completed
in 90 minutes, 60% of the same reaction would
be completed in approximately (in minutes)
_______.
(Take : log 2 = 0.30; log 2.5 = 0.40)

The number of molecules with energy greater
than the threshold energy for a reaction
increases five fold by a rise of temperature
from 27oC to 42oC. Its energy of activation in
J/mol is _____.
(Take ln 5 = 1.6094; R = 8.314 J mol–1 K–1)

It is true that :

For the reaction 2A + 3B +
\({3 \over 2}\)C
\(\to\) 3P, which
statement is correct ?

The results given in the below table were
obtained during kinetic studies of the following
reaction
2A + B \(\to\) C + D

X and Y in the given table are respectively :

The following results were obtained during kinetic studies of the reaction ;
2A + B \(\to\) Products

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For the reaction, 2A + B \(\to\) products, when the concentrations 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 r...

The given plots represent the variation of the
concentration of a reactant R with time for two
different reactions (i) and (ii). The respective
orders of the reactions are :

Consider the given plot of enthalpy of the
following reaction between A and B.
A+ B \(\to\) C + D
Identify the incorrect statement.

For the reaction 2A + B \(\to\) C, the values of initial rate at diffrent reactant concentrations are
given in the table below. The rate law for the reaction is :

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For a reaction scheme \(A\buildrel {{k_1}} \over \longrightarrow B\buildrel {{k_2}} \over \longrightarrow C\),
if
the rate of formation of B is set to be zero then
the concentration of B is given by :

Decomposition of X exhibits a rate constant of 0.05 \(\mu\)g/year. How many year are required for the decomposition of 5\(\mu\)g of X into 2.5 \(\mu\)g?

For a reaction consider the plot of \(\ell\)n 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 –

In the following reaction; xA \(\to\) yB
\({\log _{10}}\left[ { - {{d\left[ A \right]} \over {dt}}} \right] = {\log _{10}}\left[ {{{d\left[ B \right]} \over {dt}}} \right] + 0.3010\)
'A' and 'B' respectively can be :

NO2 required for a reaction is produced by the decomposition of N2O5 in CCl4 as per the equation,
2N2O5(g) \(\to\) 4NO2(g) + O2(g).
The initial concentration of N2O5 is 3.00 mol L–1
and it is 2.75 mol L–1
after 30 minutes. The rate of
f...

If a reaction follows the Arrhenius equation, the plot ln k vs \({1 \over {\left( {RT} \right)}}\) gives straight line with a gradient (\(-\) y) unit.
The energy required to active the reactant is :

The reaction 2X \(\to\) B 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:

Consider the given plots for a reaction obeying Arrhenius equation (0oC < T < 300oC) : (K and Ea are rate constant and activation energy, respectively)

Choose the correct option :

For an elementary chemical reaction,

the expression for \({{d\left[ A \right]} \over {dt}}\) is

A bacterial infection in an internal wound grows as N'(t) = N0 exp(t), where the time t is in hours. A does of antibiotic, taken orally, needs 1 hour to reach the wound. Once it reaches there, the bacterial population goes down as $${{dN} \...

For the reaction of H2 with I2, the rate constant is 2.5 × 10–4 dm3
mol–1s–1
at 327°C and 1.0 dm3
mol–1
at
527°C. The activation energy for the reaction, in kJ mole–1
is : (R = 8.314 JK–1
mol–1
)

If 50% of a reaction occurs in 100 second and 75% of the reaction occurs in 200 secod, the order of this reaction is :

N2O5 decomposes to NO2 and O2 and follows first order kinetics. After 50 minutes, the pressure inside the vessel increases from 50 mmHg to 87.5 mmHg. The pressure of the gaseous mixture after 100 minute at constant temperature will be :

For a first order reaction, A \(\to\) P, t1/2 (half-life) is 10 days The time required for \({1 \over 4}\)th conversion of A (in days) is : (ln 2 = 0.693,    ln 3 = 1.1)

At 518oC the rate of decomposition of a sample of gaseous acetaldehyde initially at a pressure of 363 Torr,
was 1.00 Torr s–1 when 5% had reacted and 0.5 Torr s–1 when 33% had reacted. The order of the reaction is

The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is :
(Assume activation energy and preexponential factor are independent of
temperature; ln 2 = 0.693; R = 8.314 J mol−...

The rate of a reaction A doubles on increasing the temperature from 300 to 310 K. By how much, the temperature of reaction B should be Increased from 300 K so that rate doubles if activation energy of the reaction B is twice to that of reac...

Two reactions R1 and R2 have identical pre-exponential factors. Activation energy of R1 exceeds that of R2 by 10 kJ mol–1. If k1 and k2 are rate constants for reactions R1 and R2 respectively at 300 K, then ln(k2/k1) is equal to :
(R = 8...

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur
by a two step process shown below :
O3(g) + Cl\({^ \bullet }\) (g) \(\to\) O2(g) + ClO\({^ \bullet }\) (g) . . . . . .(i)
ki = 5.2 × 109 L mol−1 s−1
ClO$...

The rate law for the reaction below is given by the expression k [A] [B]
A + B \(\to\) Product
If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be :

Decomposition of H2O2 follows a first order reaction. In fifty minutes the concentration of H2O2 decreases
from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M, the rate of formation of O2 will be :

Higher order (>3) reactions are rare due to

For the non – stoichiometre reaction 2A + B \(\to\) C + D, the following kinetic data were obtained in three
separate experiments, all at 298 K.


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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–1 mol–1 and log 2 = 0.301)

For a first order reaction, (A) \(\to\) products, the concentration of A changes from 0.1 M to 0.025 M in 40
minutes. The rate of reaction when the concentration of A is 0.01 M is :

The rate of a chemical reaction doubles for every 10oC rise of temperature. If the temperature is raised
by 50oC , the rate of the reaction increases by about :

Consider the reaction :
Cl2(aq) + H2S(aq) → S(s) + 2H+ (aq) + 2Cl– (aq)
The rate equation for this reaction is rate = k [Cl2] [H2S]
Which of these mechanisms is/are consistent with this rate equation?
(A) Cl2 + H2S \(\to\) H+ + Cl– + Cl+ + ...

The time for half life period of a certain reaction A \(\to\) products is 1 hour. When the initial
concentration of the reactant ‘A’, is 2.0 mol L–1, how much time does it take for its concentration to
come from 0.50 to 0.25 mol L–1 if it i...

The half life period of a first order chemical reaction is 6.93 minutes. The time required for the
completion of 99% of the chemical reaction will be (log 2=0.301) :

For a reaction \({1 \over 2}A \to 2B\) rate of disappearance of ‘A’ is related to the rate of appearance of ‘B’ by the
expression

A radioactive element gets spilled over the floor of a room. Its half-life period is 30 days. If the initial
activity is ten times the permissible value, after how many days will it be safe to enter the room?

Consider the reaction, 2A + B \(\to\) products. When concentration of B alone was doubled, the half-life did not change. When the concentration of A
alone was doubled, the rate increased by two times. The unit of rate constant for this reac...

The energies of activation for forward and reverse reactions for A2 + B2 \(\leftrightharpoons\) 2AB are 180 kJ mol−1
and 200 kJ mol−1 respectively. The presence of catalyst lowers the activation energy of both (forward and reverse) reaction...

Which of the following nuclear reactions will generate an isotope?