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PODCAST

CHEMDUNN

The podcast that brings your chemistry textbook to life through lively conversations! Our dynamic hosts break down complex topics and concepts into relatable, everyday terms, making learning chemistry accessible and enjoyable for everyone—especially for those that are needing to ace that next exam. Each episode features insightful discussions about common core topics in the typical chemistry curriculum. Say goodbye to monotonous lectures. Get ready to laugh, learn, and ... maybe ... enjoy

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All Episodes

00:05:34

Topic: Chemical Equilibrium

CHEMDUNN ·

2025/10/10

This episode introduces chemical equilibrium, defining it as the point where the rate of the forward reaction equals the rate of the reverse reaction. This process is dynamic, meaning the reaction hasn't stopped, but the concentrations of all substances have become constant, though not necessarily equal. Equilibrium is indicated by a double arrow. The system's preference for either reactants or products is described as the equilibrium "lying to the left" or "lying to the

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00:06:44

Topic: Rate Comparisons

CHEMDUNN ·

2025/10/10

This episode explains rate comparisons in chemical kinetics, focusing on how the rate of change for each substance in a chemical reaction is related through the stoichiometry of the balanced equation. It introduce a general rate expression where the rate of change in concentration for each reactant and product is divided by its respective coefficient to determine the overall reaction rate. Using the synthesis of ammonia as a practical example, the episode demonstrates how to calculate the overall

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00:14:06

Topic: Integrated Rate Law

CHEMDUNN ·

2025/09/28

This episode demystifies the Integrated Rate Laws, the essential chemical kinetics equations that allow chemists to predict the exact concentration of a reactant at any given time. While standard rate laws show instantaneous speed, the integrated versions, derived using calculus, link concentration and time directly. The episodes explore the three main laws for zero-order, first-order, and second-order reactions, highlighting that each has a unique linear form. This linearity is the key analytical

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00:07:12

Topic: Bond Enthalpies

CHEMDUNN ·

2025/09/28

This episode explains how to calculate the enthalpy of a reaction (ΔHrxn) using average bond enthalpies. This method is based on the principle that breaking old bonds requires energy and forming new bonds releases energy. The core formula is ΔHrxn=Σ(bonds broken)−Σ(bonds formed), where "bonds broken" refers to the energy of the reactant bonds and "bonds formed" is the energy of the product bonds.

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00:05:43

Topic: Enthalpies of Formation

CHEMDUNN ·

2025/09/23

This episode explains how to calculate the enthalpy change of a reaction using standard enthalpies of formation, which are values representing the energy required to form one mole of a compound from its elements. The episode introduces the "products minus reactants" formula. It emphasizes a key fact: the enthalpy change of formation for any pure element in its most stable form is zero. This method offers a mathematical way to determine reaction enthalpy without needing to manipulate

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00:09:09

Topic: Calorimetry

CHEMDUNN ·

2025/09/23

This episode explains calorimetry, the science of measuring heat transfer, based on the Law of Conservation of Energy. It demonstrates how to use the formula q=m⋅c⋅ΔT to solve for unknown variables in two common scenarios. First, the specific heat of an unknown metal is determined by measuring the heat it loses to water in a calorimeter. Second, the enthalpy change of a neutralization reaction is calculated by finding the heat absorbed by the solution and converting it to a per-mole basis. The

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00:06:46

Topic: Hess's Law

CHEMDUNN ·

2025/09/23

This episode explains Hess's Law, a method for calculating the enthalpy change of a reaction by treating it as a sum of other known reactions. It presents three key rules for manipulating these equations: reversing an equation changes the sign of its ΔH, multiplying an equation by a coefficient requires multiplying its ΔH by the same number, and adding equations together means adding their ΔH values. By applying these rules to a sample problem, it demonstrates how to combine a series of

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00:03:35

Topic: Specific Heat Capacity

CHEMDUNN ·

2025/09/20

This episode provides a clear, concise summary of specific heat capacity and its use in thermochemistry. It introduces the fundamental concept that specific heat capacity, represented by the symbol c, is a measure of how much thermal energy a substance can store. The episode focuses on the key equation q=m⋅c⋅ΔT as the central formula for calculating heat transfer.

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00:07:36

Topic: Heating & Cooling Curves

CHEMDUNN ·

2025/09/20

A heating or cooling curve graphically represents the relationship between heat, temperature, and the physical state of a substance. The curve has sloped sections where the temperature changes as heat is added, and the substance remains in a single phase (solid, liquid, or gas). The formula q=mcΔT is used to calculate the heat involved in these sections. The curve also has flat plateaus where the temperature remains constant because the added heat is used entirely for a phase change, such as melting

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00:06:20

Topic: Thermochemical Equations

CHEMDUNN ·

2025/09/20

Enthalpy (ΔH) is the heat change in a chemical reaction and can be shown in two ways: either written with the equation or included as a reactant or product. A negative ΔH signifies an exothermic reaction that releases heat, which can be shown as a product in the equation. A positive ΔH signifies an endothermic reaction that absorbs heat, which can be shown as a reactant. In stoichiometry problems, the ΔH value acts as a conversion factor relating moles of a substance to the amount of heat released

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00:04:26

Topic: Energy Diagrams

CHEMDUNN ·

2025/09/20

Energy diagrams are a visual tool to understand the energy changes in chemical reactions. They map the reaction from reactants to products, with the vertical axis showing potential energy. The difference in energy between the start and end points is the enthalpy change (ΔH). A peak in the diagram represents the transition state, and the energy needed to reach it from the reactants is the activation energy (Ea). For an exothermic reaction, products are at a lower energy level than reactants,

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00:04:25

Topic: Heat Flow

CHEMDUNN ·

2025/09/20

Heat transfers in three primary ways: conduction, convection, and radiation. Conduction is direct heat transfer through physical contact, common in solids like a metal spoon in hot soup. Convection is heat transfer through the movement of fluids (liquids or gases), where warmer, less dense fluid rises and cooler, denser fluid sinks, creating a continuous flow, as seen when boiling water. Radiation is the transfer of thermal energy via electromagnetic waves, which doesn't require a medium, like

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00:08:36

Topic: Colligative Properties

CHEMDUNN ·

2025/09/20

Colligative properties are solution properties that depend on the number of solute particles, not their identity. The episode focuses on freezing point depression and boiling point elevation. In these calculations, m is molality (moles of solute per kilogram of solvent), Kf and Kb are solvent-specific constants found on a reference table, and i is the van 't Hoff factor, which accounts for how many particles a solute breaks into. For example, a non-electrolyte like glucose has i=1, while a

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00:08:37

Topic: Complete and Net Ionic Equations

CHEMDUNN ·

2025/09/20

Ionic equations provide a more accurate view of reactions in solution than a simple chemical equation. A complete ionic equation shows all dissolved ionic compounds as separate ions, while solids, liquids, and gases remain intact. From this, a net ionic equation is derived by removing spectator ions—those that remain unchanged on both sides of the reaction. The final net ionic equation shows only the species that directly participate in the reaction. These equations are crucial for understanding the

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00:07:03

Topic: Dilution

CHEMDUNN ·

2025/09/20

Dilution is the process of lowering a solution's concentration by adding more solvent while keeping the amount of solute constant. This process is governed by the equation M1V1=M2V2, where M is molarity and V is volume, with subscripts 1 and 2 referring to the initial stock solution and the final diluted solution, respectively. This formula is used to calculate the volume of a concentrated stock solution needed to achieve a desired final concentration and volume. A crucial safety rule,

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00:09:26

Topic: Real vs. Ideal Gases

CHEMDUNN ·

2025/09/20

Real gases deviate from ideal behavior under high pressure and low temperature because the assumptions of the ideal gas law break down. At high pressure, the volume of gas molecules themselves becomes significant, making the gas less compressible than predicted. At low temperature, weak attractive forces between molecules become noticeable, causing the gas to be more compressible and exert lower pressure. While the ideal gas law is an excellent model for normal conditions, understanding these

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00:07:46

Topic: Maxwell-Boltzmann Distribution

CHEMDUNN ·

2025/09/19

The Maxwell-Boltzmann distribution shows that molecules in a gas don't all move at the same speed, but rather follow a predictable statistical pattern. The curve representing this distribution shows a peak for the most probable speed and a long tail indicating that some molecules move very fast. The distribution is significantly affected by temperature, which shifts the entire curve toward higher speeds, and molecular mass, where lighter gases have a curve shifted toward higher speeds. This

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00:06:44

Topic: Graham's Law

CHEMDUNN ·

2025/09/19

Graham's Law states that a gas's rate of diffusion or effusion is inversely proportional to the square root of its molar mass. In simple terms, lighter gases move faster than heavier ones. This relationship comes from the fact that all gases at the same temperature have the same average kinetic energy, meaning a lighter molecule must move faster to have the same energy as a heavier one. The law's formula allows us to predict the relative speeds of gases. This principle applies to both

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00:07:30

Topic: Dalton's Law of Partial Pressure

CHEMDUNN ·

2025/09/19

This episode explains Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of each gas's individual pressure. This works because, at the molecular level, each gas acts independently. The episode gives examples, including collecting a gas over water, where the total pressure must be corrected for water vapor pressure. It also introduces the concept of mole fraction, where a gas's partial pressure can be calculated by multiplying its mole

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00:08:42

Topic: Kinetic Molecular Theory

CHEMDUNN ·

2025/09/18

This episode on kinetic molecular theory (KMT) explains gas behavior through five fundamental postulates. These are: gas molecules are in constant, random motion; they have negligible volume; there are no intermolecular forces between them; all collisions are perfectly elastic; and their average kinetic energy is directly proportional to absolute temperature. This framework helps explain gas laws by showing that pressure results from molecular collisions and that changes in temperature alter

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116 results

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