Chemical Kineti...

When the initial concentration of the reaction is doubled, the half-life is also doubled. The order of the reaction will be:

A substance having rate constant $$k$$ and initial concentration $$a$$ reacts according to zero order kinetics. What will be the time for the reaction to go to completion?

$$N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)+22$$ kcal. The activation energy for the forward reaction $$50$$ kcal. What is the activation energy for the backward reaction?

Raw milk sours in about 4 h at $$27^ o C$$, but in about 48 h in a refrigerator at $$17^ o C$$. What is the activation energy for souring of milk ?

$$N_2+3H_2\rightleftharpoons 2NH_3 +22$$kcal
The activation energy for the forward reaction is $$50$$kcal. What is the activation energy for the backward reaction?

For the first order reaction, $$t_{99}$$% $$= x \times t_{90}$$%, the value of $$x$$ will be: 

$$A$$ and $$B$$ are two different chemical species undergoing first order decompositions with half-life periods as $$3$$ and $$4.5$$ minutes respectively. If the initial concentrations of $$A$$ and $$B$$ are in the ratio $$1 : 2$$, The ratio $$C_{t_{(A)}}/ C_{t_{(B)}}$$ after three half-lives of $$A$$ would be:

A reaction takes place in three steps. The rate constants are $$k_{1}, k_{2}$$ and $$k_{3}$$. The over all rate constant $$k = \dfrac {k_{1}k_{3}}{k_{2}}$$. If (energy of activation) $$E_{1}, E_{2}$$ and $$E_{3}$$ are $$60, 30$$ and $$10\ kJ$$, the overall energy of activation is:

Graph between $$\log { k } $$ and $$\cfrac{1}{T}$$ is a straight line with $$OX=5,\tan{\theta}=\left( \cfrac { 1 }{ 2.303 }  \right) $$. Hence $${E}_{a}$$ will be:

The activation energy for the forward reaction $$X\rightarrow Y$$ is $$60KJ$$ $${mol}^{-1}$$ and $$\Delta H$$ is $$-20KJ$$ $${mol}^{-1}$$. The activation energy for the backward reaction $$Y\rightarrow X$$ is: