2

Question 1

also known as the general gas equation

Answer 1

Ideal Gas Law

Question 2

the pressure of a given mass of gas is inversely proportional to its volume, provided the temperature remains constant.

Answer 2

Boyle’s Law

Question 3

the volume of an ideal gas is directly proportional to the absolute temperature at constant pressure.

Answer 3

Charles’ Law

Question 4

the pressure exerted by a gas is proportional to the temperature of the gas when the mass is fixed, and the volume is constant.

Answer 4

Gay-Lusaac’s Law

Question 5

Attempts to explain the properties of gases and gas laws

Answer 5

Kinetic Molecular Theory

Question 6

Number of collisions each gas molecule encounters per second:

Answer 6

Collision Properties

Question 7

The mean distance traveled by a gas molecule between two successive collisions.

Answer 7

Mean Free Path

Question 8

The state of a gas can be defined using variables such as volume, temperature, pressure, and number of moles. P = f (V,T,n)

Answer 8

Equation of state

Question 9

Conditions wherein the difference between gas and liquid starts to disappear (T2-106 Perry’s 9th Ed.)

Answer 9

Critical Constant

Question 10

Substances behave alike at the same reduced states. (Principle of Corresponding States)

Answer 10

Reduced Conditions

Question 11

A dimensionless factor that describes how much a real gas deviates from ideal behavior. It indicates the ability of a gas to be compressed at a certain condition.

Answer 11

Compressibility Factor (Z)

Question 12

actual/effective pressure

Answer 12

fugacity

Question 13

is a measure of chemical potential in the form of adjusted pressure

Answer 13

fugacity

Question 14

relates to the tendency of a substance for one substance to prefer one phase over another

Answer 14

fugacity

Question 15

tendency to flee or escape; fugacity/pressure ratio

Answer 15

Fugacity Coefficient (∅)

Question 16

indicates a change in temperature upon change in pressure
(pressure drop) of a gas at constant enthalpy

Answer 16

Joule-Thomson Coefficient (𝜇JT)

Question 17

deals with the concepts of heat and temperature and the inter-conversion of heat and other forms of energy.

Answer 17

Thermodynamics

Question 18

coined the term thermodynamics

Answer 18

William Thomson (1749)

Question 19

region containing energy and/or matter that is separated from its surroundings

Answer 19

● System

Question 20

everything that interacts with the system

Answer 20

Surroundings

Question 21

closed surface surrounding a system through which energy and mass may enter or leave the system

Answer 21

System Boundary

Question 22

If A and C are in thermal equilibrium, and B and C are in thermal equilibrium, then A and B are in thermal equilibrium.

Answer 22

Zeroth law

Question 23

Energy cannot be created or destroyed, but it can be transferred.

Answer 23

First Law

Question 24

The state of entropy of the entire universe, as an isolated system, will always increase over time in the course of spontaneous change..

Answer 24

Second Law

Question 25

states that the entropy of a perfect crystal at a temperature of zero Kelvin (absolute zero) is equal to zero.

Answer 25

Third Law

Question 26

measurement of energy in a thermodynamic system. The quantity of __________ equals the total heat content of a system, equivalent to the system’s internal energy plus the product of volume and pressure.

Answer 26

Enthalpy

Question 27

amount of heat required to change its temperature by one degree

Answer 27

Heat Capacity

Question 28

thermal mass of the object and is defined as the energy in Joules required raising the temperature of the given object by one degree Celsius.

Answer 28

Heat Capacity

Question 29

represents the amount of energy in a system that is not available to do work and is often associated with the second law of thermodynamics

Answer 29

Entropy

Question 30

is a thermodynamic quantity that combines enthalpy (H) and entropy (S) to determine the spontaneity of a chemical reaction. It is defined by the formula:

Answer 30

Gibbs Free Energy

Question 31

during a reaction can predict if the reaction is spontaneous or nonspontaneous. It is given by:

Answer 31

change in Gibbs free energy

Question 32

If ΔG is negative (ΔG < 0), the reaction occurs naturally without needing external energy.

Answer 32

Spontaneous Reaction:

Question 33

If ΔG is positive (ΔG > 0), the reaction requires external energy input to proceed.

Answer 33

Non-Spontaneous Reaction

Question 34

A uniform state of matter in chemical composition and physical state; examples: gasses, crystals, miscible liquids, ice; single-phase (e.g., gasses) vs. two-phase (e.g., ice and water).

Answer 34

Phase

Question 35

Uniform macroscopic scale but not microscopic; regions of one component within a matrix of another.

Answer 35

Dispersion

Question 36

Chemical species in a system; e.g., water and ethanol are two constituents.

Answer 36

Constituents

Question 37

A chemically independent species in a system;

Answer 37

Component

Question 38

The number of independent variables you can change without affecting the number of phases in equilibrium.

Answer 38

Variance

Question 39

You can change both pressure and temperature independently without affecting the equilibrium. Thus, F = 2. The system has two degrees of freedom (the system is bivariant).

Answer 39

Single-Phase, Single-Component System

Question 40

such as liquid and its vapor: Changing temperature requires a corresponding change in pressure to maintain equilibrium, and vice versa. Thus, F = 1. The system has one degree of freedom.

Answer 40

Two Phases in Equilibrium, Single-Component System (C=1, P=2),

Question 41

Neither temperature nor pressure can be changed without disturbing the equilibrium. Thus, F = 0. The system has no degrees of freedom.

Answer 41

Three Phases in Equilibrium, Single-Component System (C=1, P=3):

Question 42

→ Developed the phase rule, a key principle in chemical thermodynamics.

Answer 42

Josiah Willard Gibbs

Question 43

describe physical and chemical equilibria over a range of different compositions,

Answer 43

Phase diagrams

Question 44

A single-phase region is usually represented

Answer 44

area

Question 45

pressure-temperature relationship for a two-phase, one-component system, assuming an ideal vapor phase and negligible molar volume of the condensed phase compared to the vapor.

Answer 45

Clausius – Clapeyron Equation

Question 46

Solutions with heat of mixing equal to zero and the volume of the solution is the sum of the volumes of the components of the solution.

Answer 46

Ideal Solutions

Question 47

law of thermodynamics.

Answer 47

Raoult’s Law

Question 48

raoult's law. who and when

Answer 48

François-Marie Raoult, 1887

Question 49

A solvent’s partial vapor pressure in a solution (or mixture) is equal or identical to the vapor pressure of the pure solvent multiplied by its mole fraction in the solution.

Answer 49

Raoult's LAw

Question 50

It states that the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of the gas:

Answer 50

Henry’s Law

Question 51

Henry’s Law. who and when

Answer 51

William Henry

Question 52

A proportionality constant that depends on the specific gas-liquid combination and temperature. It quantifies the solubility of the gas in the liquid at a given temperature. (T2-22 Perry’s 9th Ed.)

Answer 52

Henry's Constant

Question 53

Henry's law constant varies with temperature.

Answer 53

Temperature Dependence

Question 54

it is dependent on the solute-to-solvent ratio but not on the solute’s identity.

Answer 54

Boiling Point Elevation

Question 55

colligitive property of solutions that is generally proportional to the molality of the added solute

Answer 55

Freezing Point Depression

Question 56

solute particles hinder the vaporization of pure solvent

Answer 56

Vapor Pressure Lowering

Question 57

Properties that depend on the number of solute particles and the nature of the solvent

Answer 57

Colligative Properties

Question 58

pressure needed to prevent the transport of solvent particles to a more concentrated solution through semi-permeable membrane

Answer 58

Osmotic Pressure

Question 59

study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction

Answer 59

Electrochemistry

Question 60

produces electricity as the result of the spontaneous reaction occurring inside it.

Answer 60

Galvanic Cell

Question 61

a technique that uses direct electric current to drive a non-spontaneous chemical reaction

Answer 61

Electrolysis

Question 62

non-spontaneous reaction is driven by an external source of current

Answer 62

Electrolytic Cell

Question 63

total charge (Q) in coulombs that passes through the cell is proportional to the absolute amount of analyte

Answer 63

Faraday's LAw

Question 64

is a branch of chemistry that deals with the separation, identification and composition of matter

Answer 64

Analytical chemistry

Question 65

type of analysis that reveals the components of the sample.

Answer 65

Qualitative Analysis

Question 66

type of analysis that determines the amount of components present in the sample.

Answer 66

Quantitative Analysis

Question 67

deals with the measurement of the mass of a substance that is chemically related to the analyte.

Answer 67

Gravimetric Method

Question 68

measures the volume of the solution necessary to react completely with the analyte.

Answer 68

Volumetric Method

Question 69

measures the electromagnetic radiation produced by the analyte or its interactions with it.

Answer 69

Spectroscopic Method

Question 70

measures the electrical properties of the analyte such as current, potential, resistance, and amount of charge

Answer 70

Electroanalytic Method

Question 71

is the process of lowering the concentration of a solute in a solution by adding more solvents to the solution

Answer 71

Dilution

Question 72

represents how much of the original stock solution remains in the entire solution.

Answer 72

dilution factor

Question 73

It is a method in analytical chemistry to determine the quantity of an analyte based on the mass .

Answer 73

Gravimetric Analysis

Question 74

also called as neutralization titration

Answer 74

Acid-Base Titration

Question 75

usually used to find the amount of a known acidic or basic substance through acid base reactions.

Answer 75

Acid-Base titrations

Question 76

solution with an unknown molarity.

Answer 76

analyte (titrand)

Question 77

solution with a known molarity that will react with the analyte.

Answer 77

reagent (titrant)

Question 78

Addition of another chemical that changes color at the pH equal to the equivalence point, when the acid and base are in stoichiometric proportions.

Answer 78

INDICATOR

Question 79

Recording the pH as you add titrant, and if the analyte is a weak acid or base you can determine its Ka or Kb.

Answer 79

POTENTIOMETRIC

Question 80

One of the oldest analytical techniques and is often termed as argentometric titration

Answer 80

Precipitation Titration

Question 81

Involves the formation of precipitate during the titration technique

Answer 81

Precipitation Titration

Question 82

- The titrant reacts with the analyte and forms an insoluble substance called

Answer 82

precipitate

Question 83

Used for determination of halides (chloride, bromide, and iodide)

Answer 83

Volhard’s method

Question 84

Designed for the direct titration of silver in dilute nitric acid with standard thiocyanate solution. Added ferric ion forms the clear, red colored ion [FeSCN]2+, at the precipitation endpoint.

Answer 84

Volhard’s method

Question 85

This method uses the reaction between the precipitate formed and indicator. The indicator used is dichlorofluorescein which acts as an anion in solution

Answer 85

Fajan’s method

Question 86

Determines the chloride ion concentration of a solution by titration with silver nitrate.

Answer 86

Mohr’s method

Question 87

- Endpoint is reached when the reddish brown color remains ‘stable’ - does not disappear with stirring

Answer 87

Mohr's Method

Question 88

a reaction that forms a "complex"

Answer 88

Complex Formation Titration

Question 89

have high accuracies and offer the possibility of determinations of metal ions at the millimole levels

Answer 89

Complex Formation Titration

Question 90

(accepting an unshared pair of electrons; the Lewis acid, generally metallic cations),

Answer 90

metal ion

Question 91

can donate a pair of unshared electrons; Lewis base / a complexing agent; can be a neutral molecule such as water or ammonia; or an ion such as chloride, cyanide, or hydroxide

Answer 91

ligand

Question 92

can also be called Ethylenediaminetetraacetic acid (EDTA) Titration

Answer 92

Complex Formation Titration

Question 93

Formation of permanent faint turbidity.

Answer 93

Liebig Method

Question 94

has two electrodes, which are immersed in an electrolyte solution.

Answer 94

Electrochemical Cell

Question 95

use to prevent the two solutions from mixing

Answer 95

Salt bridge

Question 96

the electrode where reduction occurs (Red Cat)

Answer 96

Cathode

Question 97

the electrode where oxidation occurs (An Ox)

Answer 97

Anode

Question 98

stores electrical energy. The reaction is spontaneous and allows flows of electrons from the anode to the cathode with the aid of an external conductor

Answer 98

Galvanic or voltaic cells

Question 99

an electrochemical cell that requires an external source of electrical energy to operate. Reaction is not spontaneous

Answer 99

Electrolytic cell