Test: Integrated Rate Equations(7 Nov) - JEE MCQ

The correct answer is Option C
For a first-order reaction, the half-life is given by: t_1/2 = 0.693/k

For zero order reaction the rate equation is [A] = -kt + [Ao]

Thus the slope of the line is -ko

The correct answer is option  B
t_1/2​ = k0.693​
    = 0.693​/(6.2 × 10^{− 4})​ = 1117.7s

The correct answer is option D
Units:- for K can be calculated by (Mole)^1-n (Litre )^n-1 Time ^-1...
Here,n is the order of the reaction ....
On substituting n = 1.
We get, K units as;
K = (Mole)^1-1( Litre)^1-1 sec^-1.
K=sec-1.......

The correct answer is option A
As we know, for a first order reaction,

The correct answer is Option A
For first order reaction, the half-life period is independent of initial concentration.
For first order reaction, the half-life period expression (t1/2) is given by the expression t1/2= , where k is the rate constant.

The half life of a reaction is 15 min
So,
Here we go..
Formula to be used :

K =0.693/t = 0.693/15
__= 0.462/10 = 0.0462 min^-1

The correct answer is Option B.

For exothermic reaction, ΔH<0
E_b = E_f + ∣ΔH∣ or
E_f < E_b

The ratio of the rate constant of a reaction at two temperatures differing by 10⁰C is called temperature coefficient of reaction.

• Definition: The Arrhenius equation describes the relationship between the rate constant of a reaction and the temperature at which the reaction occurs.


• Formula: The Arrhenius equation is given by: k = A * e^(-Ea/RT), where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the ideal gas constant, and T is the temperature in Kelvin.


• Effect of Temperature: As per the Arrhenius equation, an increase in temperature leads to an increase in the rate constant of the reaction. This is because higher temperatures provide the reactant molecules with more energy, allowing them to overcome the activation energy barrier more easily.


• Application: The Arrhenius equation is widely used in chemical kinetics to predict how changes in temperature will affect the rate of a reaction.