Chemical Kinetics

Short Answer Type

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A spontaneous reaction is not necessarily a fast reaction. Why?

A spontaneous reaction means that it has tendency to occur of it self, giving enough time, without side intervation it simply predicts the direction of reaction or feasibility of reaction and not at all the rate of the reaction.
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    In some cases it is found that a large number of colliding molecules have energy more than threshold value, yet the reaction is slow. Why?
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    For reaction NO2 + CO → CO2 + NO, the rate law is Rate = k[NO2]2. How many molecules of CO are involved in slowest process?
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    Define activation energy of a reaction.
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    State any one condition under which a bimolecular reaction may be kinetically of first order.
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    The reaction 2H2(g) + O2(g) --> 2H2O(g) is feasible. How is that hydrogen and oxygen mixture allowed to stand at room temperature shows no formation of water at all?
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    How is half period related to initial concentration for a second order reaction?
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    A order of reaction is found to be zero. Will its molecularity be zero?
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    The rate constant of a reaction is 3 x 102 h–1. What is the order of reaction?
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    Why is instantaneous rate preferred over average rate of reaction?
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