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Cooling Curve ​ ​ A graphical representation of the relationship between temperature and time as a substance cools.

The rate of the reaction can be defined as either: Grade 10 SABIS ​ The quantity of products produced per unit time OR the quantity of reactants consumed per unit time.

Reaction of alkali metal hydride with water: Grade 10 SABIS ​ Generally: MH(s) + H2O(l) → M+ (aq) + OH- (aq) + H2(g) Observations for the reaction of alkali metal hydride with water: Evolution of a gas that burns with a squeaky pop sound with a lit splint.

< Back Previous Next 💎🔬 Purification 🔬💎 Purification involves using electrolysis to remove impurities from a metal. For instance, in the purification of copper: The cathode (-ve electrode) is pure copper. The anode (+ve electrode) is impure copper. The electrolyte is aqueous copper (II) sulfate. During electrolysis, copper ions (Cu2+) in the electrolyte are reduced (gain electrons) at the cathode and become solid copper atoms. Meanwhile, solid copper atoms at the anode are oxidized (lose electrons) and become copper ions (Cu2+), entering the electrolyte. This maintains the electrolyte's concentration, as the ions being deposited on the cathode are replaced by the ions from the anode. Any impurities in the anode copper do not dissolve and fall to the bottom. ⚗️🧪 Electroplating 🧪⚗️ Electroplating is a process that uses electrolysis to coat a metal object with a thin layer of another metal. The primary purposes of electroplating are to enhance the object's appearance and to protect it from corrosion. In a typical electroplating process: The cathode (-ve electrode) is the object to be electroplated. The anode (+ve electrode) is the metal used for coating (for example, silver). The electrolyte is a solution containing ions of the metal used for coating (for example, silver nitrate). As electrolysis proceeds, metal ions from the electrolyte are reduced at the cathode and become solid metal atoms, adhering to the object's surface. Meanwhile, at the anode, the metal is oxidized and releases ions into the electrolyte, maintaining its concentration. It's crucial to ensure the object to be electroplated is clean and entirely immersed in the electrolyte. Also, rotating it can help achieve an even coating. Regarding your reference to a past paper question (Specimen 2023, 2, q30), could you provide more context or the actual question? Unfortunately, I can't access specific past papers beyond my knowledge cut-off in September 2021. However, I'd be more than happy to help if you could provide more details about the question! Press Next for the next lesson

Microscopic changes that take place when a solid is warmed Grade 10 SABIS ​ When a solid is warmed in thermochemistry, several microscopic changes occur at the molecular level. These changes involve the increased kinetic energy of the solid's constituent particles and their interactions, leading to observable macroscopic effects such as expansion, changes in lattice structure, and phase transitions. As the solid is heated, the temperature of the system rises, and this increase in temperature corresponds to an increase in the average kinetic energy of the solid's particles. The particles, which may be atoms, ions, or molecules, gain energy and vibrate more vigorously around their fixed positions within the solid's lattice structure. The increased kinetic energy causes the intermolecular or interatomic forces within the solid to weaken. These forces, such as ionic bonds, metallic bonds, or covalent bonds, hold the particles together in a highly organized lattice arrangement. As the particles gain energy, the forces become less effective at maintaining the lattice structure's rigidity. The weakened intermolecular or interatomic forces result in thermal expansion of the solid. The increased vibrational motion of the particles causes them to move slightly farther apart, leading to an increase in volume. This expansion is commonly observed when solids are heated. In addition to expansion, the increased kinetic energy can lead to changes in the lattice structure of the solid. For example, in some cases, the solid may undergo a phase transition from one crystal structure to another as the temperature increases. This transition involves rearrangements of the particles within the lattice, resulting in a change in the solid's physical properties. Furthermore, at higher temperatures, some solids may undergo melting, where the particles gain sufficient energy to overcome the intermolecular or interatomic forces completely. This transition from a solid to a liquid phase involves the disruption of the lattice structure and the conversion of the solid into a mobile liquid state. It's important to note that the microscopic changes in a solid being warmed are reversible. When the solid is cooled, the particles lose kinetic energy, and the intermolecular or interatomic forces regain their effectiveness, leading to a decrease in volume and a return to the initial state. Understanding the microscopic changes that occur when a solid is warmed is crucial in thermochemistry and various applications. It allows us to analyze energy transfers, phase transitions, and the behavior of substances under different temperature conditions. In summary, when a solid is warmed in thermochemistry, microscopic changes take place at the molecular level. The increased kinetic energy of the particles weakens the intermolecular or interatomic forces, resulting in expansion, changes in lattice structure, and, in some cases, phase transitions. Recognizing and studying these microscopic changes enhances our understanding of energy transfer and the behavior of solids at different temperatures.

Enthalpy Change (ΔH) Grade 10 SABIS ​ Enthalpy change, represented as ΔH, is a concept in thermochemistry that describes the difference in heat content between the products and reactants of a chemical reaction. Think of it as the "energy difference" before and after a reaction occurs. Imagine you have a candle burning. The wax and oxygen react to produce carbon dioxide and water vapor. The enthalpy change, ΔH, represents the energy released or absorbed during this combustion process. Now, consider making a cup of tea. When you add hot water to a tea bag, the enthalpy change represents the heat energy transferred to the water, causing it to dissolve the tea compounds and produce a flavorful beverage. In everyday life, we experience enthalpy changes when cooking. For example, when you bake a cake, the enthalpy change occurs as the batter transforms into a delicious, fluffy dessert due to the energy released during the chemical reactions between the ingredients. Similarly, when you boil water on the stovetop, the enthalpy change indicates the energy absorbed by the water molecules, causing them to gain heat and eventually reach the boiling point. Enthalpy change is crucial for understanding the heat effects in chemical reactions. For instance, in hand warmers, the chemical reaction inside generates an enthalpy change, releasing heat and providing warmth on cold days. In summary, enthalpy change (ΔH) represents the energy difference before and after a chemical reaction. It influences everyday scenarios like cooking, brewing tea, and even hand warmers. By studying enthalpy changes, we can comprehend the heat transfers and energy transformations that occur in various processes around us.

The decomposition of water into H2 and O2 gas Grade 10 SABIS SABIS Endothermic

Recognize different formats of expressing heat of reaction Grade 10 SABIS ​ The heat of reaction (∆H) represents the amount of heat energy gained or lost during a chemical reaction. It can be expressed in different formats depending on the specific information provided. Let's analyze each option and identify the equivalent equations for the given reaction: a) N2(g) + 2O2(g) → 2NO2(g) ΔH = +68 kJ: This equation is an equivalent representation of the given reaction. It explicitly states that the heat of reaction (∆H) is +68 kJ, indicating that the reaction releases 68 kJ of heat energy. c) 1⁄2N2(g) + O2(g) → NO2(g) ΔH = + 34 kJ: This equation is also an equivalent representation of the given reaction. It differs from the original equation by using the stoichiometric coefficients to balance the reaction. It shows that the heat of reaction (∆H) is +34 kJ, indicating the release of 34 kJ of heat energy. d) N2(g) + 2O2(g) → 2NO2(g) ΔH = +68 kJ/mol N2: This equation is another valid representation of the given reaction. It includes the molar quantity of nitrogen gas (N2) and specifies the heat of reaction (∆H) per mole of nitrogen gas. It indicates that for each mole of N2, the heat of reaction is +68 kJ. f) N2(g) + 2O2(g) → 2NO2(g) ΔH = +34 kJ/mol NO2: This equation is also an equivalent representation of the given reaction. It includes the molar quantity of nitrogen dioxide (NO2) and specifies the heat of reaction (∆H) per mole of nitrogen dioxide. It indicates that for each mole of NO2, the heat of reaction is +34 kJ. The remaining options (b) and (e) are not equivalent to the given reaction: b) N2(g) + 2O2(g) → 2NO2(g) ΔH = -68 kJ: This equation incorrectly states that the heat of reaction (∆H) is -68 kJ, suggesting that the reaction absorbs 68 kJ of heat energy. This contradicts the given information of the reaction releasing heat energy. e) 1⁄2N2(g) + O2(g) → NO2(g) ΔH = −34 kJ: This equation incorrectly states that the heat of reaction (∆H) is -34 kJ, indicating that the reaction absorbs 34 kJ of heat energy. Again, this contradicts the given information of the reaction releasing heat energy. In summary, the equivalent equations to the given reaction N2(g) + 2O2(g) + 68 kJ → 2NO2(g) are options a), c), d), and f). These equations accurately represent the given reaction and provide information about the heat of reaction (∆H) in various formats, including the heat change per mole of N2 or NO2.

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Atomicity Definition General ​ Atomicity is the term used to describe the number of atoms bonded together within a molecule. It represents the smallest unit of a compound that retains the chemical properties of that substance. Explanation with examples from here

Condensation of steam Grade 10 SABIS SABIS Exothermic