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Free CBSE - Class 12 Chemistry - Chemical Kinetics worksheets

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1.

The following data were obtained during the first order thermal decomposition of \(SO_{2}Cl_{2}\) at a constant volume. \(SO_{2}Cl_{2}(g) \rightarrow SO_{2}(g) + Cl_{2}(g)\) 

Calculate the rate of the reaction when total pressure is 0.65 atm.

2.

The rate constant for the decomposition of \(N_{2}O_{5}\) at various temperatures is given below:

Draw a graph between \(ln k\) and \(1/T\) and calculate the values of \(A\) and \(E_{a}\). Predict the rate constant at 30° and 50°C.

3.
The rate constant for the decomposition of hydrocarbons is \(2.418 \times 10^{-5}s^{-1}\) at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.
4.
Consider a certain reaction \(A \rightarrow Products\) with \(k = 2.0 \times 10^{-2}s^{-1}\). Calculate the concentration of \(A\) remaining after 100 s if the initial concentration of \(A\) is \(1.0 mol L^{-1}\).
5.
Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law, with \(t_{1/2} = 3.00\) hours. What fraction of sample of sucrose remains after 8 hours ?
6.
The decomposition of hydrocarbon follows the equation
\(k = (4.5 \times 10^{11}s^{-1}) e^{-28000K/T}\)
Calculate \(E_{a}\).
7.
The rate constant for the first order decomposition of \(H_{2}O_{2}\) is given by the following equation:
\(log k = 14.34 – \frac{1.25 \times 10^{4}K}{T}\)
Calculate \(E_{a}\) for this reaction and at what temperature will its half-period be 256 minutes?
8.
The decomposition of \(A\) into product has value of \(k\) as \(4.5 \times 10^{3} s^{-1}\) at 10°C and energy of activation \(60 kJ mol^{-1}\). At what temperature would \(k\) be \(1.5 \times 10^{4}s^{-1}\)?
9.
The time required for 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the value of \(A\) is \(4 \times 10^{10}s^{-1}\). Calculate \(k\) at 318K and \(E_{a}\).
10.
The rate of a reaction quadruples when the temperature changes from 293 K to 313 K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.
- OR -

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