Acetone undergoes photodissociation upon absorption of 330nm light. Exposure of a gaseous sample of acetone to a radiant power of 20mW at 330nm for a period of 3 hours results in the photodissociation of 75 µmol of acetone. The quantum yield for the photodissociation, assuming all the light is absorbed, is

Substance ‘A’ is exposed to 600nm, 100 W light source for 6626s, with 50% of the incident light being absorbed. ‘A’ decomposes according to the reaction A→B . As a result of irradiation, 0.2 mol of B is produced. The quantum yield of the reaction is closest to

The concentration (C) of a compound undergoing decomposition as a function of time (t) is given below:​

The order of the reaction is

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​For a reaction, raising the temperature from 200K to 300K results in the increase of rate constant by a factor of 2. The activation energy for this reaction in kJ mol^-1 is closest to (ln2=0.69). 

For the reaction, ​

the equilibrium constant is 0.16 and k₁ is 3.3×10^-4s^-1.​The experiment is started with pure cis from. The time taken for half the equilibrium amount of trans isomer to be formed is about

The rate constant for the reaction, A₂B₄O→AB₄ +AO is described as, $$\log k = 14.1 - \frac{10000 \, \text{K}}{T}$$. The activation energy for this reaction (in kJ mol^-1) is closest to

The rate of decomposition of a gas is $$10\, \mathrm{mM}\, \mathrm{s}^{-1} \text{ when } 10\% \text{ is reacted and it is } 5\, \mathrm{mM}\, \mathrm{s}^{-1} \text{ when } 40\% \text{ is reacted.}$$ ​The order of the reaction is:

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The effective activation energy for the reaction:

$$\text{A} + \text{B} \xrightleftharpoons[k_a']{k_a} \text{I} \xrightarrow{k_b} \text{P}$$

with the following potential energy versus reaction coordinate plot is

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A protein has 3 tyrosine residues and ‘n’ tryptophan residues both of which are the only amino acids absorbing at 280nm. If the absorbance of the protein having a concentration of 

in a cuvette of path length 2 cm) is 0.59, the number of tryptophan residues in the protein must be

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The effective rate constants for a gaseous unimolecular reaction:

​following the Lindemann-Hinshelwood mechanism are

​respectively. The rate constant for the activation step in the mechanism is approximately equal to (in

​

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The predicted rate law, using the steady state approximation, for the reaction 

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