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    Chemical Kinetics
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    What is the difference between order and molecularity of a reaction?

    Molecularity

    Order of a reaction

    1. It is the total number of molecules of the reactants taking part in a single step of the reaction.

    1. It is the sum of the indices to which the concentration terms are raised in rate equation, for the reaction.

    2. It is always a whole number.

    2. It may be a whole number, a fraction or zero.

    3. It is obtained from the simple balanced chemical equation.

    3. It is obtained through experimentation and is dependent upon the rate for the overall reactions.

     

    4.It is theoretical concept.

    4. It is experimental quantity.
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    Identify, giving reasons, the faster reaction in the following:
    C(s)+2H2O(g)→ 2H2(g) + CO2(g)
    C(s)+2H2O(s)→Catalyst 2H2(g) + CO2(g)
    C(s)+2H2O(s)→Catalyst 2H2(g) + CO2(g)

    The reaction carried in the presence of catalyst is fast because in the catalysed reaction the activation energy needed is less as compared to the uncatalysed reaction.
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    Identify, giving reasons, the faster reaction in
    the following:

    C(s)+1/2 O2(g) →500° CO(g)C(s) + 1/2 O2(g) →1000°CO(g)
    The second reaction is fast because the increase in temperature increases the number of effective collisions among the reacting species.
    121 Views
    Answer
    Identify, giving reasons, the faster reaction in the following:
    2Na(s) + I2(s) → 2Nal(s)
    2Na(s)+I2(g) → 2Nal(s)
    2Na(s)+I2(g) → 2Nal(s)
    The second reaction is expected to be fast because iodine molecules in the gaseous state have greater surface area and more kinetic energy than the molecules in the solid state.
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    Answer
    Identify, giving reasons, the faster reaction in the following:

    N2(10 atm) + 3H2(10 atm) → 2NH3(g)N2(5 atm) + 3H2 (5 atm) → 2NH3(g)
    The first reaction will proceed at a fast speed because under high pressure the number of reactant molecules per unit volume are more compared with low pressure. This means that when the pressure is high, the collisions among the reactant molecules are more and as a result, the chemical reaction will be fast compared with low pressure. 
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