Chemical Kineti...

The rates of most reactions doubled when their temperature is raised from $$298\ K$$ to $$308\ K$$, calculate their activation energy?

A first order reaction goes upto 8% in 10 min. What time will it take to complete 99%

 If a reaction follows the Arrhenius equation, the plot $$lnK$$ vs $$ \dfrac{1}{(RT)}$$  gives a straight line with a gradient $$(-y)$$ unit. The energy required to activate the reactant is : 

The catalysts decrease the Ea from $$100 KJmol^-1$$ to $$80 KJmol^-1$$. At what temperature the rate of reaction in the absence of catalyst at 500 K will be equal to the rate of reaction in the presence of a catalyst .

The reaction, $$X \rightarrow Y$$ is an exothermic reaction. Activation energy of the reaction for conversation of $$x$$ into $$Y$$ is $$150kJ mol^{-1}$$. Enthalpy is $$135 kJ mol^{-1}$$. The activation energy for the reverse reaction, $$Y \rightarrow X$$ will be

Consider the following in respect of zero-order reaction
i. $${ t }_{\frac{1}{2} }$$ is directly proportional to the initial concentration
ii. Time taken for the completion of the reaction is twice its $${ t }_{ 1/2 }$$
iii. Concentration of the reactant decreases linearly with time
Which of the statements given above are correct?

If the values of enthalpies of reactants and products are p and q J/mol respectively. If the activation energy for the backward reaction is r J/mol, then the activation energy for forward reaction will be in (J/mol) (take only magnitudes)

The rate  law of the reaction A + 2B $$\rightarrow $$ product is given by $$\frac{d(product)}{dt} = k[A]^2[B]$$. If $$A$$ is taken in large excess, the order of the reaction will be:

For the decomposition of $${ N }_{ 2 }{ O }_{ 5 }(g)$$ it is given that - $${ 2N }_{ 2 }{ O }_{ 5 }(g)\longrightarrow 4{ NO }_{ 2 }(g)$$ Activation energy = Ea, $${ N }_{ 2 }{ O }_{ 5 }(g)\longrightarrow { 2NO }_{ 2(g) }+\frac { 1 }{ 2 } { O }_{ 2 }(g)$$ activation energy =$${ E }a^{ ' }$$then 

For a first order reaction, the ratio of time for the completion of 99.9% and half of the reaction is