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4ecdd6b9-602f-4945-bfee-32f6a94b2d7e Chemical kinetics SABIS Grade 10 SABIS is the study of reaction rates.

6de5efa8-0086-4f23-9235-a10af8abad04 Melting/Fusion The change of a substance from a solid to a liquid state at a specific temperature.

d2c57db7-7310-4eec-8c96-0767e3e76e39 Chemical Grade 10 SABIS SABIS Relating to chemistry or chemicals.

SABIS IGCSE A level O level Al choueifat American AP Chemistry "Discover the power of personalized chemistry tutoring with K-Chemistry. From high school to university level, our online and face-to-face tutoring, paired with a rich repository of study materials, revision resources, and practice exams, provide everything you need to excel. Trust in our experience and join millions of successful students in their chemistry journey." About Us Finding Inspiration in Every Turn Welcome to K-Chemistry your one-stop destination for all things chemistry. We offer tailored tutoring and a vast array of curated study materials for learners at all levels. Our passionate team, with its profound academic and professional background in chemistry, is committed to making your learning journey engaging and fruitful. Explore Chemistry Universe and experience the joy of unraveling the mysteries of chemistry with us. Our Story K-Chemistry was founded in 2014 by Mr. Hisham Mahmoud, a seasoned professional with a Bachelor's degree in Chemical and Pharmaceutical Sciences from Cairo, Egypt. The inspiration to create K-Chemistry came from Hisham's personal experience, witnessing many students struggling with chemistry concepts. He saw the need for a platform that could make chemistry accessible and enjoyable for everyone, regardless of their prior knowledge or skills. Over the years, K-Chemistry has undergone significant evolution to cater to a growing base of eager learners. Starting as a humble tutoring initiative, it has expanded into a comprehensive online learning hub, encompassing a wide array of study materials. During the early stages, we faced challenges in reaching out to students and convincing them about the efficacy of online learning. However, with consistent efforts, the incorporation of innovative teaching methods, and the relentless pursuit of quality, we overcame these hurdles and moved ahead. Our most notable milestone came when we crossed the mark of serving hundreds of students per year, a testament to the trust and value we have built among our learners. Students from various backgrounds and learning levels have found K-Chemistry an enriching and supportive platform, helping them gain a deep understanding of complex chemistry topics and achieve academic success. At K-Chemistry, our core values revolve around fostering a deep love for chemistry, nurturing curiosity, and building a strong foundation for our students. We believe that a solid understanding of chemistry not only contributes to academic growth but also shapes informed and innovative future scientists. Join us in this rewarding journey as we continue to demystify the fascinating world of chemistry for learners worldwide. Meet The Team Hisham Mahmoud Founder & Lead Teacher Ashley Jones Tech Lead Tess Brown Office Manager Lisa Rose Product Manager Kevin Nye HR Lead Alex Young Customer Support Lead Our Students At K-Chemistry, we cater to a diverse group of learners with varying educational needs and backgrounds. Our student community ranges from high school students who are trying to get a grip on the basics of chemistry to undergraduate and postgraduate students diving into more complex topics.

70185c86-2c67-47d7-b507-d9c30f2c1c79 6 understand that some bond energies are exact and some bond energies are averages A Level Chemistry CIE When discussing bond energies, it is important to recognize that not all bond energies are exact values. Some bond energies are known precisely, while others are represented as average values. Understanding the distinction between exact and average bond energies is essential for accurate calculations and interpretations in chemical reactions. Exact bond energies refer to situations where the energy required to break a specific bond in a particular molecule is precisely known. These values are obtained from experimental measurements or highly accurate theoretical calculations. Exact bond energies are typically available for simple diatomic molecules or stable compounds with well-defined structures. For example, the bond energy of the O-H bond in a water molecule (H2O) is an exact value because it can be directly determined experimentally. The energy required to break this specific bond in water is known with high precision. On the other hand, average bond energies represent the average energy required to break a particular type of bond in a variety of compounds. These values are obtained by considering a range of molecules that contain the same bond and calculating the average energy required to break that bond across those molecules. Average bond energies are useful when exact bond energies are not available or when dealing with more complex molecules where the specific environments and neighboring atoms can influence bond strengths. These values provide an estimation of bond energies that can be used for calculations and predictions. For example, the average bond energy of the C-C bond in organic compounds is an average value obtained from considering a variety of carbon-carbon bonds in different molecules. It represents the typical energy required to break a carbon-carbon bond in various contexts. It's important to note that average bond energies can vary to some extent depending on factors such as molecular structure, neighboring atoms, and the presence of functional groups. Therefore, they are approximate values that provide a general indication of bond strengths. In practical applications, average bond energies are often more commonly used due to the wide range of compounds encountered in chemical reactions. These values serve as valuable tools for estimating energy changes and making predictions about reaction outcomes. In summary, the distinction between exact and average bond energies is crucial in understanding the nature of bond strength. Exact bond energies are precise values obtained for specific bonds in individual molecules, while average bond energies represent the average energy required to break a particular type of bond across various compounds. Recognizing the difference allows for accurate calculations and interpretations of bond strengths in chemical reactions.

08786cd6-efb7-4e90-aa4e-e2f751206045 Exothermic Grade 10 SABIS SABIS A reaction that releases heat to the surroundings.

962aedbe-4db2-44fa-ae78-13ee1fe9d6b8 Calculate H of a reaction as Σbonds broken − Σbonds formed Grade 10 SABIS Calculating ΔH (enthalpy change) of a reaction using the sum of bonds broken minus the sum of bonds formed is a fundamental concept in thermochemistry. This method is based on the idea that the enthalpy change of a reaction is determined by the energy required to break the existing bonds in the reactants and the energy released when new bonds are formed in the products. To calculate ΔH using this approach, we start by identifying the bonds present in the reactants and the products. Each bond is associated with a specific bond energy, which represents the energy required to break that bond. The sum of bonds broken refers to the total energy required to break all the bonds in the reactants. This is determined by adding up the bond energies of all the bonds in the reactant molecules. Similarly, the sum of bonds formed refers to the total energy released when new bonds are formed in the products. This is determined by adding up the bond energies of all the bonds in the product molecules. Once the bond energies for the bonds broken and formed are determined, we subtract the sum of the bond energies of the bonds formed from the sum of the bond energies of the bonds broken. The resulting value represents the enthalpy change of the reaction, ΔH. For example, let's consider the combustion of methane (CH4) to form carbon dioxide (CO2) and water (H2O). We know the bond energies for the C-H, C=O, and O-H bonds involved in this reaction. By subtracting the sum of the bond energies for the bonds formed (C=O and O-H) from the sum of the bond energies for the bonds broken (C-H), we can calculate the enthalpy change, ΔH, for this reaction. It's important to note that the bond energies used in these calculations are typically average values and can vary depending on the specific molecular environment and conditions. Additionally, bond energy calculations assume that all bonds in a molecule have equal energy, neglecting any effects of neighboring atoms or functional groups. Calculating ΔH as the sum of bonds broken minus the sum of bonds formed provides a valuable approach to estimate the enthalpy change of a reaction without relying on direct experimental measurements. It allows us to understand the energy changes associated with the breaking and forming of chemical bonds during a reaction. In summary, calculating ΔH of a reaction as the sum of bonds broken minus the sum of bonds formed involves determining the bond energies for the bonds broken and formed in the reactants and products. By subtracting the sum of the bond energies for the bonds formed from the sum of the bond energies for the bonds broken, we can calculate the enthalpy change of the reaction. This approach provides insights into the energy transformations occurring in chemical reactions and aids in understanding the thermodynamic behavior of systems.

Concise content for Grade 12 SABIS Curriculum < 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

97549368-238f-4602-948b-8c5badfce29d Coefficient Grade 10 SABIS SABIS The number preceding the chemical symbol and indicating the quantity of particles

e5bb001d-74b3-47c2-bb84-061688fe1d75 < Back Previous Next The Periodic table Next Topic

8ab8f71e-1a76-468f-9332-0a283163e5ec Find heat involved with given mass of reactant/product from H Grade 10 SABIS Finding the heat involved with a given mass of reactant or product from ΔH (enthalpy change) is an important aspect of thermochemistry. It allows us to determine the amount of heat transferred during a chemical reaction, based on the known enthalpy change and the mass of the reactant or product. The heat involved (q) can be calculated using the equation q = ΔH * m, where q represents the heat involved, ΔH is the enthalpy change, and m is the mass of the reactant or product. To use this equation, we need to know the value of ΔH, which can be obtained from experimental data or calculated using thermochemical equations. Additionally, we need to know the mass (m) of the reactant or product involved in the reaction. For example, let's consider the combustion of methane (CH4), where the enthalpy change (ΔH) is known to be -890 kJ/mol. If we have 10 grams of methane, we can calculate the heat involved as follows: q = ΔH * m = -890 kJ/mol * (10 g / 16 g/mol) = -556.25 kJ Therefore, in this case, the heat involved with 10 grams of methane in the combustion reaction is approximately -556.25 kJ. It's important to note that the sign of the enthalpy change (ΔH) indicates the direction of heat transfer. A negative ΔH value represents an exothermic reaction, where heat is released, while a positive ΔH value represents an endothermic reaction, where heat is absorbed. It's crucial to ensure that the units of enthalpy change (ΔH) and mass (m) are consistent in the calculation. If the enthalpy change is given in kilojoules per mole (kJ/mol), the mass should be in moles as well. By using the equation q = ΔH * m, we can determine the heat involved with a given mass of reactant or product in a reaction. This calculation allows us to understand the energy changes associated with chemical reactions and provides valuable insights into the heat flow within a system. In summary, finding the heat involved with a given mass of reactant or product involves using the equation q = ΔH * m, where q represents the heat involved, ΔH is the enthalpy change, and m is the mass of the reactant or product. By multiplying the enthalpy change by the mass, we can calculate the amount of heat transferred. Understanding and calculating the heat involved are essential in studying and analyzing energy changes in chemical reactions.

92f26f48-6328-4d02-b3d9-3df42efe8753 Elements in one column have similar chemical properties. Grade 10 SABIS