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Chem 2 > Final > Flashcards

Final Flashcards

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1
Q

Voltaic (Galvanic) Cell
charge of its anode and cathode
and flow of electrons

A

A Spontaneous chemical reaction that is used to PRODUCE an electrical current.

Anode has a (-) charge
Cathode has a (+) charge

Electron Flow is from (-) to (+), anode to cathode

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2
Q

Half-Cell

A

Comprised of a metal electrode immersed in a solution coating its cation. One is anode (oxidation) and one is cathode (reduction)

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3
Q

Salt bridge

A

Connects the two half-cells and allows ions to migrate from one half-cell to the other without the solution mixing

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4
Q

a. ionic-covalent bonding, interactions (H-bonding, ion-ion, dipole, London)
b. Heat capacity problems
yes c. Colligative properties, fp depression and bp elevation
d. Calculate f..H, f..G, f..S from appropriate data and know what they mean
e. Use and find rate laws
f. Equilibrium constant Kc and how to use it 􀀲
and salts
yes g. LeChatlier Principle
h. pH, pOH calculations for strong acid, weak acid, strong base, weak base, titrations
i. Buffer system concept and calculations
J. Calculate and use Ksp

A

g. Le Chatelier’s principle can be used to predict the behavior of a system due to changes in pressure, temperature, or concentration.
Le Chatelier’s principle implies that the addition of heat to a reaction will favor the endothermic direction of a reaction as this reduces the amount of heat produced in the system.
Increasing the concentration of reactants will drive the reaction to the right, while increasing the concentration of products will drive the reaction to the left.

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5
Q

Oxidation is defined as

A

LOSS of electrons

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6
Q

Reduction is defined as

A

GAIN of electrons

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7
Q

Be able to work problems using the Combined Gas Law Equation.

A

(P1)(V1)/T1 = (P2)(V2)/T2

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8
Q

b. Be able to use reaction ratios to calculate the mass of a reactant required or mass of a product formed.
d. Be able to calculate the concentration of a solution as “molarity”.

A

a

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9
Q

Statement of Faraday’s Law and its equations

A

Amount of product formed is directly proportional to amount of electricity used

1 amp = coulomb/sec

1 mole of electrons = 6.02x 10^23

1 faraday = 96,500 coulombs

1 faraday = 1 Eq. Wt.

Eq. Wt. = (Atomic Weight) / (Electrical Charge)

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10
Q

Describe the colligative properties of solutions. Understand on what factors they depend.
Carry out calculations involving freezing point depression, boiling point elevation, and osmotic pressure.

A 
DT = iKbm for boiling
DT = iKfm for freezing
DT= change in temperature
i = the van't Hoff factor, which is the number of particles into which the solute dissociates
m = the molality, which is the moles of solute per kilograms of solvent
Kb = the molal boiling point constant (for water, Kb = 0.5121oC/m)
Kf = the molal freezing point constant (for water, Kf = -1.86 oC/m)
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11
Q

Know what factors affect reaction rates and how they affect lhe rates.
Be able to use a rate law to determine how changes in concentration will affect a rate. Know that 1hc value of k changes when (a) the temperature changes and when (b) a catalyst is added.
Be able to find the rate law for a reaction by the method of initial rates. Be able to determine the order of a reaction with respect to a particular reactant from the graphs of [reactant! vs. time, In I reactant] vs. time, or !/[reactant] vs. time.
Know the formula for and be able to calculate half-life for first order reactions.
Understand the Collision Theory of reaction rates.
Be able to define and identify activation energy and the transition state on a progress of reaction graph. Be able to identify which are endothermic and exothermic. Know how a catalyst affects the reaction rate
Know how to determine if a reaction mechanism supports a given rate law.

A

The rate law expression for a reaction with reactants A, B, etc. is:
rate = k[A]x[B]y …
where the rate constant k and the orders x, y, … must be experimentally determined.

The value of k changes when (a) the temperature changes and when (b) a catalyst is added. The rate law for a reaction is usually found by the method of initial rates.

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12
Q

Be able to work problems using the Ideal Gas Law Equation.

A 
PV = nRT
P (Pressure) in (atm, Torr, Pa, mmHg)
V (Volume) in (L,m³)
=
n (Moles) in (mol)
R (Gas Constant) in (0.082057 L atm mol-1 K-1)
T (Temperature) in (K)
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13
Q

Be able to work problems using the Ideal Gas Law Equation.

A 
PV = nRT
P (Pressure) in (atm, Torr, Pa, mmHg)
V (Volume) in (L,m³)
=
n (Moles) in (mol)
R (Gas Constant) in (0.082057 L atm mol-1 K-1)
T (Temperature) in (K)
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14
Q

What is the numerical value assigned to R, the gas constant, in (L atm mol-1 K-1)?

A

(0.082057 L atm mol-1 K-1)

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15
Q

relationship of delta G to E cell

A 
deltaG = -nFE
n= moles
F= faraday's constant
E= cell voltage
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16
Q

Statement of Faraday’s Law and its equations

1 amp to coulombs
1 mole of electrons
1 faraday to coulombs
1faraday to eq.wt.

A

Amount of product formed is directly proportional to amount of electricity used

1 amp = coulomb/sec

1 mole of electrons = 6.02x 10^23

1 faraday = 96,500 coulombs

1 faraday = 1 Eq. Wt.

Eq. Wt. = (Atomic Weight) / (Electrical Charge)

17
Q

Hess’s Law

A

The enthalpy change for a given reaction is the same whether it occurs in one step or in a series of steps. Therefore, if the heats of reaction are known for each step of a series of steps that would produce the desired products from the given reactants, then the sum of those values will be equivalent to the heat of reaction for the single step reaction.

18
Q

Relationship of delta G to E cell

A 
deltaG = -nFE
n= moles
F= faraday's constant
E= cell voltage
19
Q

Nernst Equation

A

E =E0-[.0592/n]logQ

20
Q

Nernst Equation

A

E =E0-[.0592/n]logQ

21
Q

a. Be able to calculate equilibrium constant expression for any balanced equation for a homogeneous or heterogeneous reaction, given appropriate data. Know what its magnitude means.
b. Use LeChatelier’s Principle to determine the direction in which a system at equilibrium will shift when stresses of the following kinds are applied:
(a) change in volume
(c) change in amounts of reactants or products(b) change in temperature
(d) addition of a catalyst
Be able to calculate new equilibrium concentrations after a shift has occurred.

A

aa

22
Q

Hess’s Law

A

delta H= ms delta T
m= mass
s= specific heat
The enthalpy change for a given reaction is the same whether it occurs in one step or in a series of steps. Therefore, if the heats of reaction are known for each step of a series of steps that would produce the desired products from the given reactants, then the sum of those values will be equivalent to the heat of reaction for the single step reaction.

23
Q

What is the numerical value assigned to R, the gas constant, in (L atm mol-1 K-1)?

A

(0.0821 L atm mol-1 K-1)

24
Q

Be able to use the Henderson-Hasselbalch equations to calculate the pH of buffer solutions.

A

pH=pKa + log [salt]/[acid]

pKa= -log[Ka]

25
Q

What does a buffer solution need to consist of?

A

a salt with a WEAK acid or a WEAK base

26
Q

Be able to calculate the “percent yield”

A

actual/theoretical x 100

27
Q

reaction rate

A

-delta[R]/delta t
or
delta [P]/ delta t

R= reactants
P= products
28
Q

If the collection of products is thermodynamically more stable than the collection of reactants under the given conditions, the change is said to be_______.
If not, the change is said to be_______.

A

spontaneous

non-spontaneous

29
Q

delta S equals what?

A

Entropy

delta S reaction= sum of S products - sum of S reactants

30
Q

a positive delta S means what?

A

more disorder solid to liquid

31
Q

a negative delta S means what?

A

less disorder gas to liquid

32
Q

delta G equals what?

A

delta G = delta H - T delta S
H= Change in Heat
T= Temperature (K)
S= change in disorder

33
Q

delta G equals what?

A

delta G = delta H - T delta S
H= Change in Heat
T= Temperature (K)
S= change in disorder

34
Q

If delta E for energy is positive, heat is

A

absorbed, endothermic

35
Q

If delta E for energy is negative, heat is

A

released, exothermic

36
Q

Density equals…

A

mass / volume

Chem 2 (3 decks)

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