Dependence of Rate on Concentration, Rate Expression and Rate Constant, Order of a Reaction, Molecularity of a Reaction
- Chemical Kinetics part 19 (Numerical)
undefined video tutorial00:13:45
- Rate Laws, Rate Constants, Reaction Order
undefined video tutorial00:08:58
- Chemical Kinetics part 17 (Determine rate constant,order of reaction)
undefined video tutorial00:11:06
- Chemical Kinetics part 7 (Order of reaction)
undefined video tutorial00:13:11
- Chemical Kinetics part 18 (Numerical)
undefined video tutorial00:13:53
- Chemical Kinetics part 11 (Molecularity of reaction)
undefined video tutorial00:10:40
- Chemical Kinetics part 6 (Reaction rate :Concentration)
undefined video tutorial00:19:41
The following results have been obtained during the kinetic studies of the reaction:
2A + B → C + D
|Experiment||A/ mol L−1||B/ mol L−1||Initial rate of formation of D/mol L−1 min−1|
|I||0.1||0.1||6.0 × 10−3|
|II||0.3||0.2||7.2 × 10−2|
|III||0.3||0.4||2.40 × 10−2|
Determine the rate law and the rate constant for the reaction.
Time required to decompose SO2Cl2 to half of its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.
For a chemical reaction R → P, the variation in the concentration (R) vs. time (t) plot is given as:
(i) Predict the order of the reaction.
(ii) What is the slope of the curve ?
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is (i) doubled (ii) reduced to half?
For the hydrolysis of methyl acetate in aqueous solution, the following results were obtained :
|[CH3COOCH3] / mol L–1||0.60||0.30||0.15|
(i) Show that it follows pseudo first order reaction, as the concentration of water remains constant.
(ii) Calculate the average rate of reaction between the time interval 30 to 60 seconds.
(Given log 2 = 0.3010, log 4 = 0.6021)
(a) A reaction is second order in A and first order in B.
(i) Write the differential rate equation.
(ii) How is the rate affected on increasing the concentration of A three times?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
For a reaction A + B ⟶ P, the rate is given by
Rate = k [A] [B]2
How is the rate of reaction affected if the concentration of B is doubled?
A first order reaction has a rate constant 1.15 10−3 s−1. How long will 5 g of this reactant take to reduce to 3 g?
For a reaction, A + B → Product; the rate law is given by, `r = k[A]^(1/2)[B]^2` . What is the order of the reaction?
For a reaction R ---> P, half-life (t1/2) is observed to be independent of the initial concentration of reactants. What is the order of reaction?
In a first order reaction x → y, 40% of the given sample of compound remains unreacted in 45 minutes. Calculate rate constant of the reaction.
For a reaction:
Rate = k
(i) Write the order and molecularity of this reaction.
(ii) Write the unit of k.
The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?
The following data were obtained during the first order thermal decomposition of SO2Cl2 at a constant volume :
SO2Cl2 (g) → SO2 (g) + Cl2 (g)
Calculate the rate constant.
(Given : log 4 = 0.6021, log 2 = 0.3010)
For the first order thermal decomposition reaction, the following data were obtained:
Time / sec Totalpressure / atm
Calculate the rate constant
(Given: log 2 = 0.301, log3 = 0.4771, log 4 = 0.6021)