Chemical Reactions and the Theory of Collisions Quiz

Study Notes

A pastilla efervescente (effervescent tablet) does not react in the air but reacts instantly when put in beer water due to the presence of various substances that can react violently when they come into contact under certain conditions.
Max Strauss and William Louis independently explained the rapidity of chemical reactions in the early 20th century, interpreting it as the frequency of collisions between reactant molecules, their energy upon collision, and their colliding orientation.
Without proper conditions, there's no reaction between reactants, as in the case of wood and sawdust reacting with oxygen in the air, despite a large amount of reactant molecules.
The theory of collisions states that for two substances to react, their particles must collide and result in either no or a chemical change, known as an ineffective or effective collision, respectively.
In an effective collision, reactant molecules' chemical bonds break, and new bonds form, producing new products.
The reaction in cold water occurs slowly because the reactant molecules and water molecules move slowly, leading to few and insufficiently energetic collisions.
In hot water, however, reactions occur quickly due to faster-moving, more energetic water molecules and reactant molecules.
The reaction rate can be expressed as a collision factor 'f', which describes how many of these collisions result in a reaction, formed by two parts: collision energy and reactant molecule orientation.
Keeping certain medications in a dry place is recommended due to a better understanding of why iron rusts more easily in water and why gases need a spark or flame to activate the reaction, which is called combustion.

Description

Test your knowledge on chemical reactions, collision theory, reaction rates, and factors influencing reaction speed. Learn about the importance of collision frequency, energy, and orientation in chemical reactions.