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For a reaction, A + B → Product; the rate law is given by,_13-11-08_Utpal_12_Chemistry_4_9_html_72be5927.gif){kind=small}
. What is the order of the reaction?
The order of the reaction_13-11-08_Utpal_12_Chemistry_4_9_html_3d801889.gif){kind=small}
_13-11-08_Utpal_12_Chemistry_4_9_html_29e9d4f5.gif){kind=small}
= 2.5
The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?
The reaction X → Y follows second order kinetics.
Therefore, the rate equation for this reaction will be:
Rate = k[X]2 (1)
Let [X] = a mol L−1, then equation (1) can be written as:
Rate1 = k .(a)2
= ka2
If the concentration of X is increased to three times, then [X] = 3a mol L−1
Now, the rate equation will be:
Rate = k (3a)2
= 9(ka2)
Hence, the rate of formation will increase by 9 times.
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