Chemical Kineti...

The most common molecular collisions are in between:

The half life of first order reaction $$PCl_{5} \rightarrow PCl_{3}+Cl_{2}$$ is 10 minutes at a certain temperature. The time in which the concentration of $$PCl_{5}$$ would be reduced to 10% of the initial concentration is:

For the gas phase decomposition $$A\rightarrow2B$$, the rate constant is $$6.93\times 10^{-3}$$ $$min^{-1}$$ at 300K. The percentage of A remaining at the end of 300 minutes is :

The rate of a certain reaction at different times are as follows:

For a zero-order reaction $$A$$ $$\rightarrow $$ product, the rate constant is $$10^{-2}\ mol\ L^{-1}\ s^{-1}$$ . Starting with 10 moles of $$A$$ in a 1 L vessel, how many moles of $$A$$ would be left unreacted after 10 minutes?

Which is the graphical representation for the zeroth order reaction?

For the reaction $$2N_2O_5 \rightarrow 4NO_2+ O_2$$ rate at a particular time and rate constant are $$1.02\times 10^{-4}\ M s^{-1}$$ and  $$3.4\times10^{-5}\ Ms^{-1}$$ respectively. Then the concentration of $$N_2O_5$$ at that time will be:

The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, $$k = A.e^{E^{\ast }/RT}. Activation energy $$(E^{\ast })$$ of the reaction can be calculated by plotting

If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately: (log 4 = 0.60, log 5 = 0.69)