The activation energy of a reaction can be determined from the slope of which of the following graphs?

When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is

The rate of a first-order reaction is $0.04 \,$mol L$^{-1}$s$^{-1}$ at $10 \,$s and $0.03 \,$mol L$^{-1}$s$^{-1}$ at $20 \,$s$$ after initiation of the reaction. The half-life period of the reaction is (in seconds).

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below:$\newline$(i)$X_2 \rightarrow X + X$(fast)$\newline$(ii)$X + Y_2 \rightleftharpoons XY + Y$(slow)$\newline$(iii)$X + Y \rightarrow XY$(fast)$\newline$The overall order of the reaction will be

A first-order reaction has a specific reaction rate of $10^{-2}$ s$^{-1}.$ How much time will it take for 20 g of the reactant to reduce to 5 g?

The correct difference between first- and second-order reactions is that

When initial concentration of the reactant is doubled, the half-life period of a zero-order reaction

If the rate constant for a first order reaction is $k,$ the time $(t)$ required for the completion of $99\%$ of the reaction is given by:

For the chemical reaction$\\ N_2 (g) + 3H_2 (g) \rightleftharpoons 2NH_3 (g), \\$the correct relation is:

An increase in the concentration of the reactants of a reaction leads to a change in:

The rate constant for a first-order reaction is $4.606 \times 10^{-3}$ s$^{-1}.$ The time required to reduce $2.0$ g of the reactant to $0.2$ g is:

The slope of Arrhenius Plot $\ln k$ vs. $\frac{1}{T}$ of first-order reaction is $-5 \times 10^3$ K. The value of $E_a$ of the reaction is:$\newline$(Given $R = 8.314$ J K$^{-1}$mol$^{-1})$

The given graph is a representation of kinetics of a reaction. The y and x axes for zero and first-order reactions, respectively, are:

For a first-order reaction $A \rightarrow$ Products, the initial concentration of $A$ is $0.1$ M, which becomes $0.001$ M after $5$ minutes. The rate constant for the reaction in $$min$^{-1}$ is:

Given below are two statements:$\newline$Assertion A: A reaction can have zero activation energy.$\newline$Reason R: The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value is called activation energy.$\newline$In the light of the above statements, choose the correct answer from the options given below.

For a certain reaction, the rate = k[A]^2[B]. When the initial concentration of A is tripled keeping concentration of B constant, the initial rate would