Kinetics

Investigating conductivity changes during electrolysis using different salt solutions as electrolytes.

Measuring and comparing rate constants for nucleophilic substitution reactions conducted in solvents with varying viscosities.

Recording pH shifts when diluting strong acids with solvents possessing different dielectric constants.

Analyzing enthalpy changes by conducting exothermic reactions within calorimeters containing various solvent densities.

NO2 = 0, F2 = 2, Overall = 2

NO2 = 1, F2 = 2, Overall = 2

NO2 = 0, F2 = 1, Overall = 1

NO2 = 1, F2 = 2, Overall = 3

It lowers activation energy.

It decreases product concentrations.

It increases activation energy.

It raises enthalpy change (∆H) for reactions.

A catalyst raises activation energy for both types of reactions.

A catalyst lowers activation energy for endothermic but raises it for exothermic reactions.

A catalyst has no effect on activation energies for either type of reactions.

A catalyst lowers activation energy for both types of reactions.

Doubling this reactant’s concentration leads directly to quadrupling this step's observed rate when others are held steady.

Observing direct Quadruple Increase Step's Observed Rate When One Reactant Is Doubled Indicative being Second Order Respect

Halving This Reactant's Concentration results in Doubles amount Time required For Product formation To Begin Steady State Conditions Are Maintained throughout Experimentation Process Changes Observed Over Time Seem Impeccable Of Initial Concentrations involved

Doubling this Reactant’ s Concentration results In no Change In Overall Reaction Rate Under Steady conditions.

Carbon dioxide (CO₂)

Oxygen (O₂)

Hydrogen peroxide (H₂O₂)

Iodine (I₂)

Raising the temperature.

Increasing the concentration of reactants.

Reducing reactant particle size.

Adding a catalyst irrelevant to the reaction pathway.

1st

4th

3rd

2nd

k1 = 10.7 s^-1

k1 = 1.000 M8s^-1

k1 = 5403 M^0.5 * s^0.5

k1 = 1.23 x 10^-6 M^-1*s^-1

It decreases activation energy and increases kinetic energy.

It has no effect on either activation or kinetic energies but speeds up reactions by other means.

It does not change activation energy but increases kinetic energy allowing more particles to overcome it.

It increases both activation energy and kinetic energy.