Chemical Kineti...

In a reaction involving one single reactant, the fraction of the reactant consumed may be defined as $$f=\left(1-\dfrac {C}{C_{0}}\right)$$ where $$C_{0}$$ and $$C$$ are the concentrations of the reactant at the after time, t. For a first order reaction:

In a first order reaction the amount of reactant decayed in three half lives (let $$a$$ be is initial amount) would be:

If a first order reaction is completed to the extent of $$75$$% and $$50$$% in time interval, $${t}_{1}$$ and $${t}_{2}$$, what is the ratio $${t}_{1}:{t}_{2}$$?

75% of a first order reaction was completed in 32 minutes. When was 50% of the reaction completed?

For the consecutive unimolecular-type first order reaction $$A \xrightarrow{k_1} R \xrightarrow{k_2} S$$, the concentration of component $$R, C_R$$ at any time $$t$$ is given by $$: C_R = C_{AO} K_1 \left[\dfrac{e^{k_1t}}{(k_2 - k_1)} + \dfrac{e^{-k_2t}}{(k_1 - k_2)}\right]$$ if $$C_A = C_{AO}, CR = C_{RO} = 0$$ at $$t = 0$$ the time at which the maximum concentration of $$R$$ occurs is:

The time for half-life period of a certain reacting $$A\rightarrow $$ product is an hour. How much time does it take for its concentration to come from 0.50 to 0.25 mol $${ L }^{ -1 }$$ if it is a zero order reaction?

The rate constant, the activation energy and the arrhenius parameter of a chemical reaction at $${ 25 }^{ 0 }C$$ are $$3\times { 10 }^{ 14 }{ sec }^{ -1 }:\ 104.4J{ mol }^{ -1 }$$ and $$6.0\times { 10 }^{ 14 }{ sec }^{ -1 }$$ respectively, the value of the rate constant as $$T\rightarrow \infty $$ is:

In the following first-order competing reactions. 

The rate of the first order reaction is $$0.69\times { 10 }^{ -2 }mol{ L }^{ -1 }{ min }^{ -1 }$$ and the initial concentration is $$0.2mol{ L }^{ -1 }$$. The half life period is: