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Definition of the rate of reaction

the activation energy of the reaction is large

$ 0.2 \times 10 ^ {-4} $
$ { d [H_2 ] \over dt } = - 0.3 \times 10 ^ {-4} Ms^{-1} $
$ But Rate = - { 1 \over 3 } { d [ H_2 ] \over dt } = + { 1 \over 2 } { d [ NH_3 ] \over dt } $
$ Hence { d [NH_3 ] \over dt } = - { 2 \over 3} { d [H_2 ] \over dt }= - { 2 \over 3 } ( -0.3 \times 10 ^ {-4} ) = 0.2 \times 10 ^ {-4 } $

$ \triangle $ H of reaction

$ 0.012 atm min^{-1} $
$ - { d [N_2 O_4 \over dt } = + { 1 \over 2 } { d [NO_2 ] \over dt }$
$ - { (0.32 - 0.50 ) \over 30 } = 0.006 = { 1 \over 2} {d [NO_2 ] \over dt } $
$ \therefore { d [NO_2] \over dt } = 0.012 atm min^ {-1} $

$ K = K_1 / K_2 $

$ { 1 \over 6 } Rate = k [A] ^ {1/2} [A]^{1/3} [c] ^1 $
$ \therefore Order of reaction = { 1 \over 2 } + { 1 \over 3} + { 1 \over 1 } = { 11 \over 6 } $

$ Rate = K[A][B]^2 $
Keeping [B] constant, [A] is made a 4 times, rate also become 4 times. Hence rate $ \alpha [A] $
Keeping [A] constant, [B] is doubled, rate becomes 4 times.
Hence rate $ \alpha [B] ^ 2$
$ \therefore rate = K[A][B]^ 2$

$ Rate = K[A][B] ^ 2 $
Keeping [B] constant, [A] is made a 4 times, rate also become 4 times.
Hence $ rate \alpha [A] $
Keeping [A] constant, [B] is doubled, rate becomes 4 times.
Hence $ rate \alpha [B]^2 $
$ \therefore rate = K[A][B]^2$

concentration of reactants

temperature is changed

$ H_2 + Cl_2 \rightarrow 2 HCl $

$ H_2 + Br_2 \rightarrow 2 HBr $

Unimolecular reaction

any value between 1 and 3