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For a first order reaction half life period t(1/2)is independent of initial concentration of its reacting species. What is meant by half life period of a reaction?

For a first order reaction, half life does not depend on.............

For a first order reaction, derive expression for the degree of dissociation of the reactant in the exponential form.

For a first order reaction -(d[A])/(dt)=K[A]_(0), the reaction is carried out by taking 100mol//L then concentration of A decayed after time (1)/(K) is :

For a first order reaction AtoB the reaction rate at reactant concentration of 0.01 M is found to be 2.0xx10^(5)Msec^(-1). The half life period of the reaction is [Give your answere divide by 247]

For a first order reaction Ato products 93.75% of A initilly taken (2M), reacts in 80 min, then

For a first order reaction (A)to products the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is

For a first order reaction at 27^(@)C the rato of time required for 75% completion of 25% completion of reaction is

For a first order reaction ArarrB the rate constant is x "min"^(-1) . If the initial concentration of A is 0.01 M, the concentration of A after one hour is given by the expression.

For a first order reaction at 27^@C, the ratio of time required for 75% completion to 25% completion of reaction is

For a first-order reaction, Aoverset(k)toB, the degree of dissociation is equal to

For a first order reaction A to P , the temperature (T) dependent rate constant (k) was found to follow the equation log k = -(2000) (1)/(T) + 6.0 . The pre-exponential factor A and the activation energy E_(a) , respectively , are

For a first order reaction : A(g) rarr B(g) + C(g)+ D(g) Occurring at 1 bar pressure and 300 K if initial volume of the container containing only A is V_(0) and after 10 minutes it is V_(10) then average life of A will be (in minutes) :

For a first order reaction A to P, the temperature (T) dependent rate constsant (k) was found to follow the equation logk=-(2000)(1)/(T)+6.0 The per-exponential factor A and the activation energy E_(a), respectively, are

For a first order reaction (A) toproducts the concentration of A changes from 0.1M to 0.025M in 40 minutes. The rate of reaction of when the concentration of A is 0.01M is:

For a first order reaction A toproduct the rate of reaction at [A] = 0.2 mol l^(-1) is 1.0 xx 10^(-2) "min"^(-1) . The half life period for the reaction is

For a first order reaction : A to nB (with n-possibly fractional), the concentration of the product varies with time as (A_(0) is the concentration of A at time t=0).

For a first order reaction A to Bthe reaction rate at reactant concentration of 0.01 M is found to be 2.0 xx 10^(-5) mol L^(-1) s^(-1) . The half life period of the reaction is

For a first order reaction A toB the reaction rate at reactant concentration of 0.01 M is found to be2.0xx10^(-5) M sec^(-1) . The half life period of the reaction is [Give your answer divide by 347]:-

For a first order reaction AtoB the reaction rate at reactant concetration of 0.01 M is found to be 2.0xx10^(-5)mol L^(-1)s^(-1). The half life period of the reactionis

For a first order reaction A rarr Products, the rate of reaction at [A] = 0.2 M is 10^-2 mol litre^-1 min^-1. The half life period for the reaction is:

For a first order reaction A rarr B, A is optically active and B is optically inactive, and following experimental data were observed : |{:("Time","0","60 min",oo),("Optical Rotation",82^(@),22^(@),2^(@)):}| If some impurity, find optical rotation after 2 hours :

For a first order reaction (A) rarr products the concentration of A changes from 0.1 M to 0.025 M in 40 minutes . The rate of reaction when the concentration of A is 0.01 M is :

For a first order reaction A rarr product with initial concentration x " mol L'^(-1) m has a half life period of 2.5 hours. For the same reaction with initial concentration . (x/2) " mol L"^(-1) the half life is ......

For a first-order reaction

For a first order reaction

For a first order reaction ,

For a first order process, (-Ea)/(RT)value is -23.03, then value of K/A is

For a first order polymerisation reaction: nA(g) to A_(n) (g) occuring at constant volume and temperature the half-life of polymerisation of 'A' is 20 min. If the total pressure of system is 2atm at t=0 "and" 1.2 "atm at" t= 20 "min". then the value of 'n' is :

For a first order process A toB, rate constant k_1 = 0.693 "min"^(-1) & another first order process Cto D , k_2 = x "min"^(-1). If 99.9% of C to D requires time same as 50% of reaction A toB , value of x?

For a first order homogeneous gaseous reaction Ato2B+C, if the total pressure after time t was P_(t) and after a long time (to to oo) was P_(oo) then k in terms of P_(t),P_(oo) and t is

For a first order decomposition of N_(2)O_(5)(g) to give NO_(2)(g)and O_(2)(g), what will be the rate constant if at initial instant, after 10 minutes and after a very long time, tolal pressure is 200 mm of Hg, 325 mm of Hg and 450 mm of Hg?

For a first order chemical reaction : A rarr P. The correct statement(s) is/are :

For a f-orbital the values of m_l are

For a diprotic acid, which of the following is true for 1^(st) and 2^(nd) ionization constants (K_(a_(1)) and K_(a_(2)))

For a disproportionationreaction the onlycorrect combination is -

For a dilute solution , Raoult's law states that:

For a dilute solution, Raoult's law states that:

For a dilute solution , Raoult.s law states that:

For a dilute solution having molality m of of a given solute in a solvent of mol.wt.M,b.pt. T_(b) and heat of vaporisation per mole DeltaH:[(aT_(b)/(am)]_(mrarr0) is equal to :

For a dilute solution of a strong electrolyte, which of the folllowing facts is correct?

For a dilute solution, lowering of vapour pressure prop mole fraction of the solute or, lowering of vapour pressure = K xx mole fraction of the solute, where K is

For a dilute solution having molality m for a given solute in a solvent of mol. Wt. M,b.pt. T_(b) and heat vaporisation per mole DeltaH, [(delT_(b))/(delm)]_(mrarr 0) is equal to

For a decomposition reaction, the values of rate constant k at two different temmperature are given below: k_(1)=2.15xx10^(-8)"L mol"^(-1)s^(-1) at 650 K k_(2)=2.39xx10^(-7)"L mol"^(-1)s^(-1) at 700 K Calculate the value ofactivation energy for this reaction. [R=8.314JK^(-1)"mol"^(-1)]