Chemical Equilibrium and Reaction Rate Factors

Le Chatelier's Principle and Equilibrium

The forward reaction is exothermic, while the reverse reaction is endothermic (depending on the specific system). According to Le Chatelier's Principle, increasing the temperature favors the endothermic reaction. In this scenario, the forward reaction is favored, and the equilibrium moves from left to right, producing more CO. Therefore, high temperature is more favorable for the production of CO.

Regarding pressure, increasing pressure favors the side with fewer moles, while decreasing pressure favors the side with more moles.

Factors Influencing Reaction Rates

A chemical reaction will speed up if the frequency of the reacting particles increases and the proportion of the particles with energy greater than the activation energy increases. Concentration, temperature, and pressure all affect the equilibrium state.

Key Factors Affecting Reaction Speed

• Concentration: Increasing the concentration of reactants leads to more collisions due to the increased number of reactant particles, hence increasing the rate.
• Particle Size: The smaller the particle size, the greater the surface area, which increases the likelihood of collisions.
• Pressure: Increasing pressure reduces the volume of gas particles, which increases the rate of collisions between particles.
• Temperature: The higher the temperature, the higher the kinetic energy of particles, causing them to move faster and collide more frequently.
• Catalysts: Catalysts provide an alternative reaction pathway with lower activation energy, hence increasing the reaction rate.

Types of Catalysts and Industrial Applications

Homogeneous Catalysts

Examples include nitrogen oxide in the lead chamber process for the manufacture of sulfuric acid, and alcohol acting as a catalyst in the oxidation of sodium sulfite solution to sodium sulfate.

Heterogeneous Catalysts

• Iron: Acts as a catalyst in the Haber process for manufacturing NH₃.
• Manganese(IV) Oxide: Used in the preparation of oxygen from hydrogen peroxide.
• Vanadium(V) Oxide or Platinized Asbestos: Used in the contact process for the manufacture of sulfur trioxide.
• Nickel (Ni), Palladium (Pd), or Platinum (Pt): Used in the catalytic hydrogenation of unsaturated hydrocarbons.

Photochemical Reactions

Photochemical reactions are initiated by the absorption of energy in the form of light. Unlike other reactions, these do not depend on heat or pressure but require light as a necessary activation energy for reactions to take place. The brighter the light (visible or ultraviolet), the faster the reaction. If the intensity of light is greater, more reactant molecules gain the required activation energy, leading to a faster reaction speed.