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MCAT > MCAT General Chemistry Part 2 > Flashcards

MCAT General Chemistry Part 2 Flashcards

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MCAT flashcards
1
Q

How does the kinetic molecular theory define a gases pressure?

A

A gases pressure is due to the collisions of the molecules with the walls of the container and all collisions are elastic

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2
Q

Because all molecules of a gas move at a constant speed between collisions and the collisions are elastic, the molecules of gas experience___

A

NO intermolecular forces

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3
Q

The average kinetic energy of a gas molecules is directly proportional to ___

A

Absolute temperature (in Kelvin) of the sample

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4
Q

The hypothesis that equal volumes of different gases at the same temperature and pressure contain the same number of particles

A

Avogadro’s hypothesis

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5
Q

A statement of the relationship between the pressure and volume of a constant amount of gas at constant temperatures

P = 1/V

A

Boyle’s Law

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6
Q

The process by which a gas escapes through a pinhole into a region of lower pressure

A

Effusion

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7
Q

The theory that states heat is associated with the thermal motion of particles, taking into account the important assumptions that individual gas molecules take up no volume and collisions between gas molecules are perfectly elastic

A

Kinetic-molecular theory

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8
Q

A gas that deviates from the behavior predicted by the ideal gas law. Real gases differ from the expected behavior of an ideal gas (lower V and P) for two reasons:

  1. The force of attraction between the particles in a gas are not zero
  2. The volume of the particles in a gas is not zero
A

Real gas

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9
Q

A reaction in which the rate is proportional to the concentration of a single reactant raised to the first power rate = k[A]

A

first-order reaction

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10
Q

used to describe the relationship between the rate of a step in a chemical reation and the concentration of one of the reactants consumed in that step

A

Order

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11
Q

What three things affect and determine the reaction rate?

A
  1. How frequently the reactant molecules collide
  2. The orientation of the colliding molecules
  3. Their energy
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12
Q

A blend of two or more metallic elements

A

Alloy

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13
Q

The process in which a bulk solid or liquid breaks up into individual molecules or ions diffuse throughout a solvent

A

Dissolution

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14
Q

Why are solids and liquids not included in equilibrium constants or expression?

A

Their concentration does not change

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15
Q

The value of the equilibrium constant (Keq) is constant at a given __

A

temperature

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16
Q

If the concentrations of reactants and products is at equilibrium then Q =

A

Keq

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17
Q

A system at equilibrium will try to neutralize any imposed change in order to reestablish equilibrium

A

Le Chateliers principle

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18
Q

The solubility of gases in liquid tends to ___ with increasing temperature

A

Decrease

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19
Q

The solubility of gases in liquids tends to ___ with increasing pressure

A

Increase

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20
Q

All group 1 elements and ammonium (NH4+) are ___

A

soluble

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21
Q

All nitrate (NO3-), perchlorate (CLO4-) and acetate (C2H3O2-) are___

A

soluble

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22
Q

All silver (Ag+) lead (Pb2+/4+) and mercury (Hg2+) are ___ unless they are part of nitrates, perchlorates, or acetates

A

Insoluble

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23
Q

The extent to which a salt will dissolve in water can be determined from its __

A

solubility product constant Ksp

24
Q

The __ is the reaction quotient for a solubility reaction

A

Qsp ionic product

25
Q

If Qsp < KsP

A

more salt can be dissolved

26
Q

If Qsp = Ksp

A

Solution is saturated

27
Q

If Qsp > Ksp

A

Excess salt will precipitate

28
Q

A compound that dissociates when it dissolves in water to give the H+ ions

A

Arrhenius acid

29
Q

A compound that dissociates when it dissolves in water to give the OH- ion

A

Arrhenius base

30
Q

Any molecule or ion that can donate an H+ (proton)

A

Bronsted-Lowry acid

31
Q

Any molecule or ion that can accept an H+ (proton)

A

Bronsted-Lowry base

32
Q

The amount of acid or base a buffer solution can absorb without significant changes in pH

A

buffer capacity

33
Q

What are the 6 most common strong acids with a Ka above 1?

A 
Hydroiodic acid
Hydrobromic acid
Hydrochloric acid
Perchloric acid HClO4
Sulfuric acid H2SO4
Nitric Acid HNO3
34
Q

What are the common strong bases (memorize these)

A

Group 1 hydroxides (NaOH)
Group 1 oxides (example: Li2O)
Some group 2 hydroxides= Ba(OH)2, Sr(OH)2, Ca(OH)2
Metal amides: NaNH2

35
Q

The conjugate base of a strong acid__

A

has no basic properties
example:
HCl +H20 -> H30+ + Cl-

36
Q

The conjugate base of a weak acid___

A

is a weak base

37
Q

The site of oxidation in a galvanic or electrolytic cell

A

Anode

38
Q

The electrode towards which anions flow through a salt bridge

A

Anode

39
Q

A set of electrochemical cells connected in series or parallel

A

Battery

40
Q

The site of reduction in a galvanic or electrolytic cell

A

Cathode

41
Q

The electrode in an electrochemical cell towards which cations flow through a salt bridge

A

Cathode

42
Q

A measure of the driving force behind an electrochemical reaction

A

Cell-potential

43
Q

A type of electrochemical cell that has identical reactants in each half reaction, but at different concentrations, thus driving a weak electrical current

A

Concentration cell

44
Q

A process in which an electrical current is used to drive a nonspontaneous chemical reaction

A

Electrolysis

45
Q

A nonspontanoeous electrical cell in which electrolysis is done

A

Electrolytic cell

46
Q

A statement of the relationship between the amount of electric current that passes through an electrolytic cell and the amount of product formed during electrolysis.

The amount of chemical change is proportional to the amount of electric current that flows through the cell

A

Faraday’s law of electrolysis

47
Q

An electrochemical cell that uses a spontaneous chemical reaction to do work, synonymous with voltaic cell

A

Galvanic cell

48
Q

A measure of the driving force behind an electrochemical reaction that is reported in units of volts

A

Potential

49
Q

Anions from the salt bridge of the galvanic cell go to the ___ and cations travel in the opposite direction

A

Anions from the salt bridge go to the anode

Cations from the salt bridge go to the cathode

50
Q

Tables on the MCAT for half-reaction potentials usually only given for ___ reactions

A

Reduction, to get the oxidation, just flip the sign

51
Q

The free-energy change for a redox reaction in which cell voltage is E is given by the equation

A

G = - nFE

n is number of moles of electrons transferred
F is faraday constant which is 96,500 coulombs
E is cell voltage V

52
Q

The redox reaction in a cell will be spontaneous if the cell voltage is __

A

positive because that will make G negative, spontaneous

53
Q

The more negative the reduction potential

A

The weaker the reactant is as an oxidizing agent, and the STRONGER the product is as a reducing agent

54
Q

The more positive the reduction potential,

A

the stronger the reactant is as an oxidizing agent, and the weaker the product is as a reducing agent

55
Q

A ___ uses an external voltage source, such as a battery, to create an electric current that forces a nonspontaneous redox reaction to occur

A

Electrolytic cell

56
Q

How do you solve for for the amount of electricity (in coulombs, C) that flowed through a cell?

A

Q = IxT

Q = charge
I = current (amps)
T (time)

MCAT (45 decks)

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