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In the reaction $ A ---> B $ . When the concentration of A is changed from 0.1 M to 1 M, the rate of reaction increases by a factor of 100. The order of reaction with respect to A is ….
2 concentration increased = 10 $ times rate increased = 10^ 2 times $ $ \therefore \; Order = 2 $
For the reaction of $ A + B --> C + D$ , doubling the concentration of both the reactants increases the reaction rate by 8 times and doubling the initial concentration of only B simply doubles the reaction rate. The rate law for the reaction is
$ r = K [A]^2 [B] (i) r = k [A] ^x [B]^y (ii) 8r = k [2A] ^x [2B] ^ y (iii) 2r = k [A] ^x [2B] ^ y $ $ z(iii) \div (i) \cong 2^y = 2 \therefore y = 1 $ $ (ii) \div (i) \cong 2 ^x = 4 \therefore x = 2 $
The unit of rate constant for a zero order reaction is
$ mole litre^ {-1} sec ^ {-1} rate = K [R] ^ n , K = { rate \over [R]^ n } = { M/s \over M^n } n = 0 $ $ K = M^{1-n} S^{-1} \therefore K = M/S $
The rate constant of a reaction has same units as the rate of reaction. The reaction is of ...
$ zero order K = { rate \over [R]^n } K = rate , when \;n = 0 $
The rate constant of reaction is $ 3 \times 10^{-3} bar^{-1} sec^{-1} $ . The order of reaction is ...
$ 2 K = { rate \over [R]^n } = { bar /s \over bar^n } when n = 2 , k = bar ^ {-1} S^{-1} $
Which of the following statements is incorrect about the molecularity of a reaction ?
There is no difference between order and molecularity of a reaction.
For a single step reaction $ A + 2B ---> Products $ , the molecularity is
3
Which of the following statement is false ?
Both order and molecularity of a reaction are always the same.
If ‘a’ is the initial concentration of the reactant, the time taken for completion of the reaction, it if is of zero order, will be
a/k For Zero order reaction $ t = { 1 \over k} { [A]_o - [A] } But [A]_o = a $ And when reaction complete $ [A] = 0 \therefore t = { a \over k } $
The reaction $ 2O_3 ---> 3O_2 $ proceeds in two steps as follows. (i) $ O3 --> O_2 + O (fast) $ (ii) $ O + O_3 --> 2O_2 (slow) $ The rate law expression should be...
$ r = k [O_3]^2 [O_2] ^ {-1} From slowest step r = k [ O_3 ] [O] $ $ From eq (i) keq = [O_2] [O] / [O_3 ] $ $ \therefore [O] = Keq [O_3] / [O_2] _2 $ $ \therefore r = k [O_3] Keq [O_2] = K^1 [O_3]^2 [O_2]^{-1} $
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