Chemistry Chemical Kinetics

Zero order reaction is always multi step reaction

From I&II, rate∝ [B]². From I&III, rate∝ [A]¹.
From IV: 7.2e-2 = k (X) (0.2)². From II: 2.4e-2=k (0.1) (0.2)². X=0.3.
From V: 2.88e-1=k (0.3) (Y)². k=2.4e-2/ (0.1*0.04)=6.
2.88e-1 = 6 (0.3)Y². Y²=0.16. Y=0.4.

Successful collisions help in the formation of new products, whereas in unsuccessful collisions the molecules just bounce back without causing any reaction. In such cases, the reaction fails and no new product or bond is formed.

For a collision to happen, the molecules must collide with each other at a high frequency. But the result can still lead to disappointment. This is because even if molecules collide effectively, they also need to be aligned properly in symmetry. Only this can help in the formation of new bonds. Hence, the molecular orientation is considered important in he concept of collision theory.

Here are a few useful applications of this concept in our day to day lives:

• Preservation and Cooking of Food
• Chemical Manufacturing
• Pharmaceuticals
• Thermometer
• Biology Enzymes
• Electrical Appliances