Temperature remains unchanged or decreases slightly as altitude is increased?

Collision theory 

- In order for a successful collision to occur, they must collide with the right amount of energy, and in the right orientation

       - Not all collisions are effective, only those that meet the minimum activation energy are effective

- The reaction rate also depends on how frequently reactant molecules collide

        - By colliding more often, reactant particles have more opportunities to undergo effective collisions

INCREASE CONCENTRATION OF REACTANTS: 

- More Particles, More Collisions: Higher concentration means more reactant molecules packed into the same volume.

- Increased Frequency: With more particles, the number of collisions occurring per second goes up significantly.

- More Successful Collisions: A greater number of total collisions increases the likelihood of collisions with sufficient energy and correct orientation (activation energy) to break bonds and form products, speeding up the reaction. 

INCREASED TEMP 

- Increases kinetic energy of the molecules, particles begin to move faster, they collide into each other more often therefore increasing frequency of collisions, there’s a higher chance of them colliding with the right amount of force and right orientation to cause a successful collision 

CATALYST

- According to collision theory, a chemical reaction occurs only when particles collide with sufficient energy to overcome the activation energy and with the correct orientation. A catalyst speeds up a reaction by providing an alternative reaction pathway with a lower activation energy. This does not increase the total number of collisions, but it increases the proportion of collisions that have enough energy to be successful (more molecules meet the minimum energy requirement and are successful). As a result, the rate of both the forward and reverse reactions increases equally. Because equilibrium depends on the relative rates of these reactions and not their absolute speeds, the equilibrium position remains unchanged, although equilibrium is reached more quickly.

VOLUME AND PRESSURE (EFFECTS ON EQUILIBRIUM) 

- If pressure increased, volume decreases

         - Reaction favours the side with less moles 

- If volume is increased and pressure is decreased

         - Reaction favours the side with more moles