Advertisements
Advertisements
Question
Write a condition under which a bimolecular reaction is kinetically first order. Give an example of such a reaction. (Given : log2 = 0.3010,log 3 = 0.4771, log5 = 0.6990).
Advertisements
Solution
\[\ce{ C_12 H22O11 + H2O ->[H+] C6 + \underset{Glucose}{C6H12O6} + \underset{Fructose}{C6H12O6} }\] Rate=K[C12H22O4]
Biomolecular reaction is Kinetically first order. Consider a chemical reaction between two substances when one reactanct is present in large excess.
`CH_3 COOC_2H5 +H_2O -> CH_3OOH + C_2H_5OH`
t=0 0.01mol 10mol 0 0
t 0mol 9.9mol 0.01 0.01 mol
Rate = K[CH3COOC2H5]
`Rate = K[CH_3COOC_2H_5] where K=K' [H2O]` the reaction behaves as first order reactions.
APPEARS IN
RELATED QUESTIONS
Consider the reaction
`3I_((aq))^-) +S_2O_8^(2-)->I_(3(aq))^-) + 2S_2O_4^(2-)`
At particular time t, `(d[SO_4^(2-)])/dt=2.2xx10^(-2)"M/s"`
What are the values of the following at the same time?
a. `-(d[I^-])/dt`
b. `-(d[S_2O_8^(2-)])/dt`
c. `-(d[I_3^-])/dt`
The rate constant for the first-order decomposition of H2O2 is given by the following equation:
`logk=14.2-(1.0xx10^4)/TK`
Calculate Ea for this reaction and rate constant k if its half-life period be 200 minutes.
(Given: R = 8.314 JK–1 mol–1)
What will be the effect of temperature on rate constant?
Calculate activation energy for a reaction of which rate constant becomes four times when temperature changes from 30 °C to 50 °C. (Given R = 8.314 JK−1 mol−1).
Consider figure and mark the correct option.
What happens to most probable kinetic energy and the energy of activation with increase in temperature?
In respect of the eqn k = \[\ce{Ae^{{-E_a}/{RT}}}\] in chemical kinetics, which one of the following statement is correct?
The activation energy in a chemical reaction is defined as ______.
The decomposition of N2O into N2 and O2 in the presence of gaseous argon follows second-order kinetics, with k = (5.0 × 1011 L mol−1 s−1) `"e"^(-(29000 "K")/"T")`. Arrhenius parameters are ______ kJ mol−1.
An exothermic reaction X → Y has an activation energy 30 kJ mol-1. If energy change ΔE during the reaction is - 20 kJ, then the activation energy for the reverse reaction in kJ is ______.
