Chemical Kineti...

The rate constant of the reaction $$A\rightarrow B$$ is $$0.6\times 10^{-3} \ mole \ per \ litre \ per \ second$$. If the concentration of $$A$$ is $$5 \ M$$, then concentration of $$B$$ after $$20 \ minutes$$ is:

The thermal decomposition of $$HCOOH$$ is a first-order reaction with a rate constant of $$2.4\times {10}^{-3}{s}^{-1}$$ at certain temperature. How long will it take for three-fourths of the initial quantity of $$HCOOH$$ to decompose?

In a homogeneous reaction $$A\longrightarrow B+C+D$$ the initial pressure was $${P}_{0}$$ and after time $$t$$ it was $$P$$. Expression for rate constant $$k$$ in terms of $${P}_{0},$$ $$P$$ and $$t$$ will be:

What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from $$300$$K to $$400$$K? $$(R=8.314$$ J $$mol^{-1}K^{-1}$$)

For a reaction $$X\longrightarrow\ Y$$, the graph of the product concentration (x) versus time (t) came out to be straight line passing through the origin. Hence the graph of $$\cfrac{-d[X]}{dt}$$ and time would be:

For a first order gas phase reaction: 

Consider the two equations at a particular temperature ;
$$2N_2O_5\rightarrow 4NO_2+O_2$$

In a first order reaction with time the concentration of the reactant decreases:

On increasing the temperature by $$10^{0}$$C:

The activation energy of a reaction is dependent on: