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# The unit of rate constant for the zero-order reaction is:A.)${ s }^{ -1 }$B.)${ molL }^{ -1 }{ s }^{ -1 }$C.)${ Lmol }^{ -1 }{ s }^{ -1 }$D.)${ { L }^{ 2 }mol }^{ -2 }{ s }^{ -1 }$

Last updated date: 20th Jun 2024
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Hint: The zero-order reaction can be defined as the rate of the reaction is proportional to the zero power of the concentration of reactants [R]. This means the rate is independent of the concentration of the reactant.

For a zero-order reaction:
${ Rate= }\frac { dC }{ dt } { =k\left[ { R }_{ 0 } \right] ^{ \circ } }$
${ k= }\frac { dC }{ dt } { = }\frac { concentration }{ time }$
${ k= }\frac { mol{ L }^{ -1 } }{ s }$
k =${ molL^{ -1 }{ s }^{ -1 }}$

So, the correct answer is “Option B”.

a.)The rate constant is equal to the rate of reaction when the concentration of all the reactants is taken as unity.
b.)The rate constant is nearly doubled with a rise in temperature by ${ 10 }^{ \circ }$ for a chemical reaction.
c.)Few examples of zero-order reaction are:

The photochemical reaction between hydrogen and chlorine
Decomposition of ${ N }_{ 2 }{ O }$ on a hot platinum surface.
The decomposition of ${ NH }_{ 3 }$ in the presence of molybdenum or tungsten is a zero-order reaction.
Iodination of acetone in the presence of ${ H }^{ + }$ ions.

d.)Zero-order reactions generally occur under the heterogeneous system. In such a system, the reactant is adsorbed on the surface of a solid catalyst, where it is converted into a product. The fraction of the surface of the catalyst covered by the reactant is proportional to the concentration of a reactant at low values. However, after a certain concentration limit of the reactant, the reaction rate does not change i.e. rate becomes independent of concentration and the reaction becomes zero order.

Note:
The possibility to make a mistake just a little portion of the reactant particles are in an area or state wherein they can respond, and this division is consistently recharged from the bigger pool.