In gaseous reactions important for the understanding of the upper atmosphere H2O and O react bimolecularly to form two OH radicals. H for this reaction is 72kJ at 500 K and Ea is 77 kJ mol-1, then Ea for the bimolecular recombination of two OH radicals to form H2O and O is:
1. 3 kJ mol-1
2. 4 kJ mol-1
3. 5 kJ mol-1
4. 7 kJ mol-1
For a reaction A Product, rate law is . The concentration of A left after time t when is:
For an exothermic chemical process occurring in two steps as;
(ii) XAB (Fast)
The progress of the reaction can be best described by:
4. All of the above.
For the non-stoichiometric reaction 2A + B C +D, the following kinetic data were obtained in three separate experiments, all at 298 K.
|Initial Concentration (B)||Initial rate of formation of C (mol L-1 S-1)|
|0.1 M||0.1 M|
|0.1 M||0.2 M|
|0.2 M||0.1 M|
The rate law for the formation of C is:
1. d[C]/dt = k[ A][B]
2. d[C]/dt = k[ A]2[B]
3. d[C]/dt = k[ A][B]2
4. d[C]/dt = k[ A]
For the reaction N2 + 3H2 2NH3, the rate = 2 x 10-4 M s-1 .Therefore, the rate is given as:
1. 10-4 Ms-1
2. 104 Ms-1
3. 10-2 sM-1
4. 10-4 sM-1
If 'I' is the intensity of absorbed light and 'c' is the concentration of AB for the photochemical process AB + hv→ AB *, the rate of formation of AB * is directly proportional to:
Which curve represents zero order reaction?
In a reaction, the rate expression is, rate = K[A][B]2/3[C]0 , the order of reaction is:
The rate of a reaction get doubles when the temperature changes from 7°C to 17°C. By what factor will it change for the temperature change from 17°C to 27°C?
In the Arrhenius equation K = Ae-Ea/RT, the quantity e-Ea/kT is referred as:
1. Boltzmann factor.
2. Frequency factor.
3. Activation factor.
4. None of the above.