NEET Chemistry Questions: Chemical Kinetics

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What is the temperature at which archeobacteria can survive ?




Archeobacteria, also known as archaea, are extremophiles that can survive in extreme conditions, including high temperatures. They thrive in environments such as hot springs and hydrothermal vents, where temperatures can reach as high as 110 °C. Therefore, the correct answer is 'All of these' as archeobacteria can survive at 90 °C, 100 °C, and 110 °C.
To keep constant time, watches are fitted with balance wheel made of........




Because dimension of invar does not vary with temperature.
Rate of reaction is defined as




Definition of the rate of reaction
The rate of reaction of spontaneous reaction is generally very slow. This is due to the fact that..




the activation energy of the reaction is large
$N_2 + 3H_2 \rightleftharpoons 2NH_3$ For the reaction the rate of change of concentration for hydrogen is $ -0.3 \times 10^{-4}Ms^{-1} $. The rate of change of concentration of ammonia is ...




$ 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 } $
Does not affect the rate of reaction.




$ \triangle $ H of reaction
In the reaction $N_2O_{4(g)} \rightarrow 2NO_{2(g)} the pressure of N_2O_4 falls from 0.5 atm to 0.32 atm is 30 minutes, the rate of appearance of NO_{2(g)} $ is




$ 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} $
In the reaction $K_1 and K_2$ are the velocity constants for the forward and backward reaction respectively. The equilibrium constant is




$ K = K_1 / K_2 $
For the reaction A + B + C --> Products, Rate = $ K[A]^{1/2 } [B]^{1/3} [C]$ . The order of reaction is




$ { 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 } $
$ A + 2B ---> C + D $ For a reaction from following data correct rat law = Mole (A) 1 0.1 2 0.3 3 0.3 4 0.4 $ liter ^ {-1} $ (B) 0.1 0.2 0.4 0.1 mole lite-1 min-1 $ 6.0 \times 10^{-3} $ $ 7.2 \times 10^{-2} $ $ 2.88 \times 10^{-1} $ $ 2.4 \times 10^{-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$
In the reaction $ A + B --> Products $ , the doubling of [A], increases the reaction rate to four times, but doubling of [B] has no effect on the reaction rate. The rate expression is ….




$ 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$
A zero order reaction is one whose rate is independent of ….




concentration of reactants
The rate constant of a reaction changes when ...




temperature is changed
Which of the following is a reaction of zero order ?




$ H_2 + Cl_2 \rightarrow 2 HCl $
Which of the following is a reaction of fractional order ?




$ H_2 + Br_2 \rightarrow 2 HBr $