Thermochemistry

It increases the number of molecules that can overcome the activation energy barrier.

It decreases the overall enthalpy change of the reactants and products.

It lowers the activation energy necessary for reactants to form products.

It changes an endothermic reaction into an exothermic one.

Initial reactants in their ground state

Formation of final products with released heat

Intermediate compounds in exothermic transition phase

Transition state leading to endothermic step

Addition of a catalyst.

Higher concentration of reactants.

Increased temperature of the system.

Stronger bonding in the reactants.

It causes immediate shift rightward entire potential curve owing additional space occupied non-reactive entities thereby increasing distance traveled particles per unit time prior interaction

It reduces frequency effective collisions among reacting molecules thus possibly affecting position peak representing activated complex

Insertion extra gaseous component may enhance overall speed dynamic interchange no impact whatsoever shape location peaks valleys depicted graphical representation

Adding inert substance leads direct reduction amount usable space confined environment results heightened speed particle movement eventual rise apex barrier needs overcome

Thermal energy.

Activation energy.

Kinetic energy.

Potential energy.

The forward reaction's threshold energy level decreases, reducing overall activation energy needed as predicted by Le Chatelier’s Principle when pressure increases due to reduced volume

Activation energy for the forward reaction would decrease but remain unchanged for reverse action since pressure favors formation of fewer moles gas-phase products typically formed in exothermic processes

It would raise both reactants' and products' energy levels while maintaining their relative difference caused by ΔHₑₓₒₜʜᴇʀᴍɪᴄ.

Activation energies for both directions increase equally because increased collisions at higher pressures make transitions harder despite any shifts in equilibrium positions

They increase temperatures at which reactions take place

However they lower overall yields from given processes

They reduce activation energies needed for reactions making them quicker

Airborne agents speed-up breaking bonds amongst substrates only

Nitrogen (N)

Helium (He)

Oxygen (O)

Fluorine (F)

It raises the initial energy of reactants

It changes the overall enthalpy change of the reaction.

It lowers the activation energy without altering the overall enthalpy change.

It decreases the final energy of products

Catalysts shift equilibrium toward more reactants by decreasing their respective activation energies only.

Catalysts do not alter equilibrium positions but decrease time taken to reach it by lowering activation energies for both directions equally.

Catalysts shift equilibrium toward more products by selectively lowering their activation energies only.

Catalysts create new pathways with higher overall energy that favors neither reactants nor products changing equilibria positions drastically over time.