Kinetics

It permanently reacts with substrates, depleting enzyme availability.

It donates electrons to substrates to reduce their oxidation states.

It specifically binds to substrates and stabilizes the transition state.

It increases temperature at localized sites to speed up reactions.

It requires closer proximity between reacting molecules than other steps do.

It releases more heat upon completion than any other step in the mechanism.

It has significantly higher activation energy compared to other steps in the mechanism.

It involves formation of products more than any other step in the mechanism.

It suppresses reverse reactions while enhancing forward reactions for quicker product formation.

It increases the rates of both forward and reverse reactions equally without affecting equilibrium constants.

It increases only the rate of forward reaction, shifting the equilibrium towards products faster.

It halts both forward and reverse reactions until removed from the system by external means.

CO = Produced in the final step

HCOOH2^+ - Produced in the 1st stepand consumed in a later step

H2SO4 - Consumed in the 1st step and regenerated in a later step

HCOOH - Increase in concentration of HCOOH increased the reaction rate

It speeds up specific biochemical reactions in organisms at body temperature.

It breaks down substrates into multiple different types of molecules.

It reduces oxygen levels needed for respiration.

It denatures proteins at higher than normal body temperatures.

The poison stabilizes intermediates prolonging the lifetime of reactive species.

The poison binds at active sites preventing substrate interaction and reducing reaction rates.

The poison increases activation energy making the reaction proceed more faster.

The poison acts as a secondary catalyst further incrementing the reaction rates.

Pd increases the activation energy of the reaction

Pd absorbs the heat produced in the reaction

One of the reactants binds on the surface of Pd, introducing an alternative reaction pathway with a lower activation energy

One of the products binds on the surface of PDd, increasing the reaction rate by decreasing the concentration of products

It consumes reactant molecules.

It increases the reaction temperature.

It changes the equilibrium constant.

It lowers the activation energy.

Catalysts change ΔG° from positive to negative ensuring product formation.

Catalysts reduce overall pressure affecting gas phase reactions improving spontaneity based on ΔG°.

Catalysts increase temperature which makes ΔG° more negative for spontaneity.

Catalysts speed up reaction rate but do not affect spontaneity determined by ΔG°.

Evenly spread out texture

None of the above

Cracks and peaks

A smooth feel