Chemical Kinetics and Nuclear ChemistryHard
Question
Select the correct statements out of I, II and III for zero order reaction
I : Quantity of the product formed is directly proportional to time
II : Larger the initial concentration of the reactant, greater the half-life period
III : If 50% reaction takes place in 100 minutes, 75% reaction take place in 150 minutes.
I : Quantity of the product formed is directly proportional to time
II : Larger the initial concentration of the reactant, greater the half-life period
III : If 50% reaction takes place in 100 minutes, 75% reaction take place in 150 minutes.
Options
A.I only
B.I and II only
C.II and III only
D.I, II and III
Solution
We know for zeroth order Rxn
For (I) x = kt
For (II) t1/2 ∞ [A0] [Initial concentration]
For (III) A0 -
= k × 100 .....(i)
A0 -
= k × t .....(ii)
t =
= 150 minutes.
For (I) x = kt
For (II) t1/2 ∞ [A0] [Initial concentration]
For (III) A0 -
= k × 100 .....(i)A0 -
= k × t .....(ii)t =
= 150 minutes. Create a free account to view solution
View Solution FreeTopic: Chemical Kinetics and Nuclear Chemistry·Practice all Chemical Kinetics and Nuclear Chemistry questions
More Chemical Kinetics and Nuclear Chemistry Questions
A complex reaction 2X + Y → Z, takes place in the following two steps. $X + Y\overset{\quad K_{1}\quad}{\rightarrow}2W$,...The rate of a reaction increases four-fold when the concentration of reactant is increased 16 times. If the rate of reac...To very good approximations, the cooling of a hot body to room temperature follows first-order kinetics (in this case, h...Decomposition of A2(g) and B3(g) follows first order kinetics as follows.$${A_{2}(g) \rightarrow 2A(g);K_{1}\left( /h^{-...For the reaction A + 2B → C, rate is given by R = [A] [B]2 then the order of the reaction is...