The unit of rate constant for zero order reaction is
- ${{s}^{-1}} $
- $ mol\,{{L}^{-1}}{{s}^{-1}}$
- $ L\,mo{{l}^{-1}}{{s}^{-1}}$
- ${{L}^{2}}\,mo{{l}^{-2}}{{s}^{-1}} $
The Correct Option is B
Solution and Explanation
or $k=\frac{dx}{dt}=\frac{\operatorname{co}nc.}{time} $
$=\frac{mol{{L}^{-1}}}{s}=mol{{L}^{-1}}{{s}^{-1}} $
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Concepts Used:
Rate of a Chemical Reaction
The rate of a chemical reaction is defined as the change in concentration of any one of the reactants or products per unit time.
Consider the reaction A → B,
Rate of the reaction is given by,
Rate = −d[A]/ dt=+d[B]/ dt
Where, [A] → concentration of reactant A
[B] → concentration of product B
(-) A negative sign indicates a decrease in the concentration of A with time.
(+) A positive sign indicates an increase in the concentration of B with time.
Factors Determining the Rate of a Reaction:
There are certain factors that determine the rate of a reaction:
- Temperature
- Catalyst
- Reactant Concentration
- Chemical nature of Reactant
- Reactant Subdivision rate