List of top Chemistry Questions on Chemical Kinetics asked in TS EAMCET

For a first order reaction ($R \rightarrow P$), a plot of $\ln \frac{[R]_0}{[R]}$ on y-axis and time on x-axis gave a straight line passing through the origin. The slope of straight line is 'x'. The rate constant of this reaction is

$\text{A}\to \text{P}$ is a first order reaction. At $300 \text{ K}$ this reaction was started with $[\text{A}]=0.5 \text{ mol}\text{L}^{-1}$. The rate constant of reaction was $0.125 \text{ min}^{-1}$. The same reaction was started separately with $[\text{A}]=1 \text{ mol}\text{L}^{-1}$ at $300 \text{ K}$. The rate constant (in $\text{min}^{-1}$) now is

The half-life of a zero order reaction A $\rightarrow$ products, is 0.5 hour. The initial concentration of A is 4 mol L$^{-1}$. How much time (in hr) does it take for its concentration to come from 2.0 mol L$^{-1}$ to 1.0 mol L$^{-1}$?

For a first order decomposition of a certain reaction, rate constant is given by the equation
$\log k(s⁻¹) = 7.14 - \frac{1 \times 10^4 K}{T}$. The activation energy of the reaction (in kJ mol⁻¹) is ($R = 8.3 J K⁻¹ mol⁻¹$)
Note: The provided value for R is 8.3. We will use the more precise value R=8.314 J K⁻¹ mol⁻¹ for accuracy, as is standard.