Author Capstone Axis

Understanding Equilibrium Constants Let’s explore how to calculate and apply equilibrium constants! 1. Calculating Kc (Concentration Constant) For the reaction: \[ \text{PCl}_5 \rightleftharpoons \text{PCl}_3 + \text{Cl}_2 \] Kc is calculated as: \[ K_c = \frac{[\text{PCl}_3][\text{Cl}_2]}{[\text{PCl}_5]} \] Example: If [PCl₃] = 1.59 M, [Cl₂] = 1.59 M, [PCl₅] = 1.41 M: \[ K_c = \frac{(1.59)^2}{1.41} = […]

Chemical Equilibrium: The Balance of Reactions ⚖️ Chemical reactions can go both ways! When the forward and reverse reactions happen at the same speed, we reach dynamic equilibrium 🌀. At this point: Concentrations of reactants and products stay constant over time ⏱️. It doesn’t matter if you start with reactants or products – you’ll reach

Understanding Equilibrium in Physical Processes What is Equilibrium? 🤔 Equilibrium is a dynamic state where two opposing processes happen at the same rate, so there’s no overall change. It’s like a dance where both partners move equally fast! Types of Physical Equilibria ⚖️ 1. Solid ⇌ Liquid (e.g., Ice-Water) At 273 K and 1 atm

Understanding Dynamic Equilibrium in Chemical Reactions ⚖️ 🌟 Key Characteristics of ALL Equilibria (Physical & Chemical) When a system reaches equilibrium: 🔒 It must be a closed system at a fixed temperature. ⚡ Both forward & reverse processes happen at the same speed (dynamic but stable!). 📏 All measurable properties (like concentration, pressure, color) stay

Gibbs Energy Change and Equilibrium ✨ Key Ideas Gibbs free energy (G) helps us predict two important things about chemical reactions: 🎯 Whether a reaction happens spontaneously ⚡ How much useful work we can get from it 🧪 Equilibrium Condition At equilibrium, the system’s free energy is at its minimum, and: \[ \Delta_r G =

Different Types of Enthalpies in Reactions 🔥 Standard Enthalpy of Combustion (ΔcH°) This is the heat released per mole when a substance burns completely in oxygen, with all reactants and products in their standard states. Combustion is always exothermic (releases heat)! Examples: Butane (cooking gas): \[ \ce{C4H10(g) + \frac{13}{2}O2(g) -> 4CO2(g) + 5H2O(l)} \quad \Delta_c

Understanding Spontaneity in Chemical Reactions 🌡️ What is a Spontaneous Process? A spontaneous process occurs naturally without external help and proceeds in one direction only. Examples include gas expanding to fill a container or carbon burning in oxygen. Key points: 🔥 Irreversible: Can only be reversed by external intervention. ⏳ Rate-independent: Spontaneity doesn’t mean “fast”

Enthalpy Change in Chemical Reactions When a reaction happens, heat is either absorbed or released. We call this heat change at constant pressure the reaction enthalpy or \(\Delta_rH\). Key Rules 🔥 Exothermic reaction: Heat released → \(\Delta_rH\) is negative (e.g., burning graphite). Endothermic reaction: Heat absorbed → \(\Delta_rH\) is positive (e.g., melting ice). Measuring Heat

First Law of Thermodynamics The energy of an isolated system is constant ⚖️. For any change: \[ \Delta U = q + w \] Where: • \(\Delta U\) = change in internal energy • \(q\) = heat transferred • \(w\) = work done on the system Key ideas: • \(\Delta U\) depends only on initial

Understanding Heat and Specific Heat 🔥 Specific heat (\(c\)) is the heat needed to raise 1 gram of a substance by 1°C (or 1 K). To calculate heat (\(q\)) for any sample: \[q = c \times m \times \Delta T\] or simply \(q = C \Delta T\), where \(C\) is total heat capacity. Heat Capacity