CHEMISTRY COMMUNITY

Owen-Koetters-4I

K solely depended on ADP

Owen-Koetters-4I

the graphs are specific to a specific reactant/molecule

Owen-Koetters-4I

the overall reaction can't come to completion until the slowest step comes to completion, so this rate determines the overall rate

Owen-Koetters-4I

work is positive when it is done on the system and negative when it is done by the system

Owen-Koetters-4I

standard Gibbs energy is under standard state conditions

Owen-Koetters-4I

the species on the left is oxidized and on the right is reduced

Owen-Koetters-4I

large k indicates a fast rate and a small k indications a slow rate

Owen-Koetters-4I

because the cell potentials of the cathode and anode are equal

Owen-Koetters-4I

subtract the standard potential of the anode (left) from the standard potential of the cathode (right)

Owen-Koetters-4I

a reaction is zero order if it is independent of the concentration of reactants

Owen-Koetters-4I

you examine if work is done on or by the system

Owen-Koetters-4I

the potential outcome can be controlled by the rate of formation of product which is a kinetic factor

Owen-Koetters-4I

State functions are independent of the path taken. Gibbs energy (G), enthalpy (H), entropy (S), heat capacity, pressure, volume, and density are all examples. Work (w) and heat (q) are not state functions.

Owen-Koetters-4I

q is negative in an endothermic reaction and positive in an exothermic reaction

Owen-Koetters-4I

Compare Q and K

Owen-Koetters-4I

A solid metal has to be used as an electrode

Owen-Koetters-4I

Strong acids have higher percent ionization and as a result there is more h3o+ in solution, leading to a lower ph value

Owen-Koetters-4I

You subtract the mol of gas formed and the mol of gas reacting

Owen-Koetters-4I

If delta g is negative it will be spontaneous in the forward direction and if it is positive the reverse will be spontaneous

Owen-Koetters-4I

A catalyst isn’t used up whereas an intermediate gets formed during an elementary step then used up and does not appear in the overall reaction

Owen-Koetters-4I

It is second order if two first order reactants affect the rate constant

Owen-Koetters-4I

kelvin

Owen-Koetters-4I

Ecell=E*cell-(RT/nF)lnQ

Owen-Koetters-4I

the initial concentration cancels in the derivation

Owen-Koetters-4I

for kinetics look at how the reaction progress and for thermodynamics look at the initial and final states

Owen-Koetters-4I

the more positive potential is the reduction half reaction and the more negative is the oxidation reaction

Owen-Koetters-4I

a pourous bridge

Owen-Koetters-4I

N is the number of mol of electrons transferred.

Owen-Koetters-4I

the more negative half reaction is the anode and the more positive half reaction is the cathode.

Owen-Koetters-4I

An oxidizing agent is stronger oxidizing than its redox couple and will undergo reduction itself. A reducing agent is more stronger reducing than its redox couple and will undergo oxidation itself.

Owen-Koetters-4I

in a concentration cell the two electrodes have the same composition but different compositions. By measuring Ecell the concentration of the left electrode can be determined. If this concentration is less than at the right, then Ecell will approach 0 and the right electrode will be the cathode.

Owen-Koetters-4I

standard conditions means 1M concentration, 1 bar pressure, and at a temperature of 273.15K

Owen-Koetters-4I

voltage is a measure of the potential difference between two electrodes

Owen-Koetters-4I

you break up a full redox reactions into two separate "half reactions" that show the oxidation and reduction reactions

Owen-Koetters-4I

you include platinum because it would be used as a salt bridge in the galvanic cell

Owen-Koetters-4I

it depends on the solution. If it is an acidic solution use H+ and if it is a basic solution use OH-

Owen-Koetters-4I

x is small when its less than 10^-3 of initial concentration of acid or base

Owen-Koetters-4I

intensive properties are independent of size and extensive properties are dependent on size

Owen-Koetters-4I

isothermal reversible expansion is at constant temperature and reversible expansion is at constant pressure

Owen-Koetters-4I

isothermal compression or expansion

Owen-Koetters-4I

it depends on if you're calculating heat capacity, specific heat capacity, or molar heat capacity

Owen-Koetters-4I

extensive properties depend on the amount of material. examples are mass and volume

Owen-Koetters-4I

integral calculus is used when we don't have constant pressure

Owen-Koetters-4I

check the percent ionization. if it is smaller than 5% than the approximation is valid

Owen-Koetters-4I

averages are used for molecules that are not diatomic

Owen-Koetters-4I

The partial pressure of a reactant is decreased in this system in dynamic equilibrium. Therefore Q temporarily rises above K and the reactants are favored until Q=K. In this example this means the partial pressure of CO2 decreases until equilibrium is met.

Owen-Koetters-4I

No. The activities of liquids and solid do not affect the K value of the reaction

Owen-Koetters-4I

You calculate initial concentration/equilibrium concentration by plugging in your approximated x-value. If this value is greater than 0.05 you must solve the cubic equation.

Owen-Koetters-4I

Oftentimes H2O is in excess. Also if it H2O were to be in liquid or solid form we wouldn't include it in the ICE table, as its activity would simply be 1.

Owen-Koetters-4I

This means there are more reactants at Eq and it sits to the left

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