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Graphical Interpretation ​ ​ The representation of Boyle's Law on a graph, showing the inverse relationship between volume and pressure for a gas.

The Maxwell-Boltzman curve can be used to explain the effect of temperature on reaction rates. Grade 10 SABIS ​

Fission Reaction Grade 10 SABIS ​ A fission reaction is a type of nuclear reaction in which the nucleus of an atom splits into two smaller nuclei, releasing a large amount of energy. This process is the basis of nuclear power and atomic bombs. To understand fission reactions, let's consider an everyday example: splitting wood logs for a fire. When you use an axe or a saw to split a large log into smaller pieces, you're performing a physical fission-like process. The energy applied to the log is released as the wood splits into two or more pieces. In nuclear fission, the nucleus of an atom, such as uranium or plutonium, is bombarded with a neutron. This causes the nucleus to become unstable and split into two smaller nuclei, known as fission fragments. Along with the fission fragments, several high-energy neutrons are released. Analogously, think of a pinata filled with candy. When it is struck with a stick, the pinata splits open, releasing a shower of candies. The initial impact destabilizes the pinata, leading to the breakage and subsequent release of energy (candies) and smaller fragments. The energy released during a fission reaction is immense. It's like a powerful explosion that can generate heat, light, and shockwaves. In nuclear power plants, controlled fission reactions are used to produce heat, which then converts water into steam, driving turbines to generate electricity. Another example of fission reactions is the sun's energy production. In the sun's core, hydrogen nuclei undergo a series of fusion reactions, combining to form helium nuclei. This fusion process releases an enormous amount of energy, providing heat and light to our planet. In nuclear reactors, such as those used for generating electricity, fission reactions are carefully controlled to sustain a chain reaction. The released neutrons from one fission reaction can trigger subsequent fission reactions in other nuclei, leading to a continuous release of energy. However, it's important to note that fission reactions can also have negative consequences if not properly controlled. Uncontrolled fission reactions can lead to nuclear meltdowns or atomic bombs, where an enormous amount of energy is released in an uncontrolled and destructive manner. In summary, fission reactions involve the splitting of atomic nuclei, releasing a significant amount of energy. Examples like splitting wood logs, breaking a pinata, nuclear power plants, and the sun's energy production help illustrate the concept of fission reactions and the release of energy through controlled nuclear processes. Understanding fission reactions is crucial for both harnessing nuclear energy for peaceful purposes and ensuring the safe handling of nuclear materials.

Effect of changing pressure on rate of reaction: Grade 10 SABIS ​ if one or more of the reactants are gaseous, an increase in pressure will increase their concentration. Increasing the concentration, increases the number of particles in a given volume thus the reacting particles will collide more frequently so the number of collisions will increase per unit time, thus rate of reaction increases. Pressure can be increased by either injecting more gas or by decreasing the volume of vessel in which the reaction is occurring.

Equations with Fractional Coefficients Grade 10 SABIS SABIS Cannot be read in terms of molecules

< Back Chapter 1: Equilibrium Explore the fascinating world of chemical equilibrium and learn how it impacts various chemical reactions and processes. Chapter 1: Equilibrium - This chapter explores the concept of chemical equilibrium, which is the state in which the concentrations of the reactants and products in a chemical reaction remain constant over time. Students will learn about the equilibrium constant, Le Chatelier's principle, and how to calculate equilibrium concentrations. Previous Next Study Material Notes Part 1 Notes Part 2 Notes Part 3 Notes Part 4 Excercises 1 Excercises 2 Excercises 3 Excercises 4 As any reaction proceeds, [reactants] decreases and [products] increases. Reversible reaction: a reaction which can go both ways. Equilibrium: is the point when the [reactants] and [products] becomes constant. Equilibrium: is the point when the [reactants] and [products] becomes constant. Equilibrium is recognized by constancy of macroscopic properties in a closed system at constant temperature. Macroscopic properties are observable properties or measurable properties like pressure, concentration, color, size, volume and mass. Macroscopic properties are observable properties or measurable properties like pressure, concentration, color, size, volume and mass. Each set of equilibrium concentrations is called an equilibrium position. Steady state: indicates a situation where macroscopic properties are constant but equilibrium does not exist as the system is not closed e.g a blue Busen burner flame. Equilibrium in physical changes: Solubility of iodine Vapor pressure of water Equilibrium in chemical reactions: NO2-N2O4 system Equilibrium is dynamic in nature since at equilibrium two microscopic processes are occurring in opposite direction at the same rate resulting in no observable macroscopic changes. Equilibrium is dynamic in nature since at equilibrium two microscopic processes are occurring in opposite direction at the same rate resulting in no observable macroscopic changes. Equilibrium is dynamic in nature since at equilibrium two microscopic processes are occurring in opposite direction at the same rate resulting in no observable macroscopic changes. Adding a catalyst or a noble gas does not alter the state of equilibrium. Equilibrium may not reached in certain equilibrium system because the activation energy of the forward reaction is too high. Le Chatelier's Principle: if an equilibrium system is subjected to a change processes will occur to partially counteract the imposed change. Low temperature is required in the Haber Process for a desirable good yield and high temperature is necessary for a satisfactory rate. The compromise used industrially involves an intermediate temperature around 450°C and even then the success of the process depends upon the presence of a suitable catalyst to achieve a reasonable reaction rate. High pressures are required in the Haber Process for a good yield and a satisfactory high rate. It is expensive and dangerous to build up a pressure. A pressure of 200 atm is actually used as a compromise. Mass Action Expression: For a general reaction: αA + βB ⇆ ΥC + ΔD Mass action expression = Q = [C]γ[D]Δ[A]/α[B]β At equilibrium: mass action expression is constant and is given a special name, equilibrium constant, Keq Concentrations of solids and liquids are NOT included in the equilibrium expression. These values are constant and are incorporate in the value of Keq directly. Temperature and the nature of solvent are the only values which determine the value of the equilibrium constant. There is only one equilibrium constant for a particular system at a particular temperature but there are an infinite number of equilibrium positions Significance of value of K If reactants and products are mixed are mixed, three things may occur:  An equilibrium is established  A reaction occurs in the forward direction  A reaction occurs in the backward direction. To find out what is occurring one needs to find the value of the mass action expression, Q and compare it to Keq. a. If Q >Keq reaction is NOT at equilibrium the backward reaction is taking place (system shifts to the left). b. If Q = Keq reaction is at equilibrium No shift occurs. c. If Q

Heating water from 20°C to 80°C Grade 10 SABIS SABIS Endothermic

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< Back Sabis Grade 12 Chemistry Concise content for Grade 12 SABIS Curriculum Course content click here https://www.k-chemistry.com/all-sabis-chapters/chapter-6-sabis-grade-12-part-3 Previous Next

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Phase Change ​ ​ The transition of a substance from one state of matter to another due to changes in temperature and/or pressure.