Chemical Kineti...

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

The rate of a reaction at 200 K 100 times less than the rate at 400 K.The activation energy of the reaction is 

Rate constant of a first order reaction is $$1.15\times 10^{-5}$$. The percentage of initial concentration that remained after 1 hour is?

For a first order process $$A\rightarrow B$$ rate constant $${k}_{1}=0.693\ {min}^{-1}$$ and another first order process $$C\rightarrow D$$, $${K}_{2}=x$$ $${min}^{-1}$$. If $$99.9$$% of $$C\rightarrow D$$ requires time same as $$50$$% of reaction $$A\rightarrow B$$, value of $$x$$? (in $${min}^{-1}$$)

A reaction $$A+B\leftrightarrow C+D$$  follows the mechanism:

Raw milk sours in 4 hours at $$27^\circ C,$$ but in 40 hours in refrigerator at $$7^\circ C.$$ What is activation energy for souring of milk:

For a first order reaction, the plot of $$'t'$$ against $$log C$$ gives a straight line with slope equal to:

For the reaction : $$ NH_2COONH_4(s) \leftrightharpoons 2NH_3(g) +CO_2(g) , K_p = 3.2 \times 10^{-5}atm^3 $$
the total pressure of the gaseous products when sufficient amount of reactant is allowed to achieve equilibrium , is:

A zero-order reaction is one

The temperature coefficient of a reaction is $$2$$. When the temperature is increased from $$30^{\circ}C$$ to $$90^{\circ}C$$, the rate of reaction is increased by