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  • (a) Define order of reaction. How does order of a reaction differ from molecularity for a complex reaction? (b) A first-order reaction is

(a) Define order of reaction. How does order of a reaction differ from molecularity for a complex reaction?

(b) A first-order reaction is 50\; ^{o}/_{o} complete in 25 minutes. Calculate the time for 80\; ^{o}/_{o} completion of the reaction.

 

 

 

 
 
 
 
 

Answers (1)

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(a) Order of a Reaction: The sum of the power of the concentration of the reactants in the rate law expression is known as the order of the reaction 

Consider the general reaction 

bA+bB\rightarrow cC+dD

Rate=K\left [ A \right ]^{x}\left [ B \right ]^{y} 

Where x is order w.r.t  A and Y is order w.r.t B

Overall order =x+y

Order of  Reaction Molecularity

(1) It is the sum of the concentration terms on which the rate of reaction actually depends. 

(2) It can be fractional as well as zero.

(1) It is the number of atom ions or molecules that must collide with one another simultaneously so as to result into a chemical reaction.

(2) It is always a whole number. It cannot be zero or fractional.

(b) For a first-order reaction :

        t_{\frac{1}{2}}=\frac{0.693}{K}

        K=\frac{0.693}{t_{\frac{1}{2}}}=\frac{0.693}{25}=0.028\; min^{-1}

Now, using the first-order reaction,

K=\frac{2.303}{t}\log \frac{\left [ R_{0} \right ]}{\left [ R \right ]}

t=\frac{2.303}{0.028}\log \frac{R_{o}}{0.2R_{o}}=\frac{2.303}{0.028}log\; 5

                                            =82.25\times 0.6991=57.50\; min

 

Posted by

Sumit Saini

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