Balancing chemical equations
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Reactants are substances that interact in a chemical reaction and are written on the left side of the equation. Products are substances formed by the reaction and are written on the right side. Common symbols are used to represent elements and compounds in chemical equations. Guidelines for writing balanced chemical equations include: writing correct formulas, starting with the most abundant element, balancing polyatomic ions, balancing hydrogen and oxygen atoms, using the lowest whole number coefficients, and checking each atom is balanced.
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Chemistry is the study of matter and its composition, structure, properties, and interactions. [1] Some key concepts introduced in the document include the classification of matter as elements, compounds, or mixtures based on its chemical and physical properties. [2] Five important laws governing chemical combinations are also outlined: the law of conservation of mass, the law of definite proportions, the law of multiple proportions, Gay-Lussac's law of gaseous volumes, and Avogadro's law. [3]
Chapter 9.1: Understand Chemical Reactions
This document discusses chemical reactions and how to write balanced chemical equations. It defines physical and chemical changes, and notes that chemical changes result in new substances being formed. A chemical reaction is described as the rearrangement of atoms when bonds break and form. Signs that a chemical reaction occurred include changes in properties, energy, color, odor, state of matter. Chemical equations use symbols to represent elements and formulas for compounds. They show the reactants on the left and products on the right. For an equation to be balanced, the number of atoms of each element must be the same on both sides. The document explains how to identify the reactants and products and balance chemical equations by adding coefficients in front of the formulas and symbols.
Chemical equations
The document discusses chemical equations and balancing reactions. It provides examples of chemical equations showing the formation of glucose from carbon dioxide and water during photosynthesis, the formation of carbon dioxide from carbon and oxygen, and the formation of water from hydrogen and oxygen. It also discusses the law of conservation of mass, which states that the total mass of reactants must equal the total mass of products in a chemical reaction.
Notes chemical equations
The document discusses balancing chemical equations by following the law of conservation of mass. It explains that a chemical equation uses symbols to represent a chemical reaction, with reactants on the left side of the yield sign and products on the right. For the equation to be balanced, the number of atoms of each element must be equal on both sides after coefficients are added. This ensures the mass is also conserved, as required by the law of conservation of mass. An example demonstrates balancing the equation for the combustion of propane by adding coefficients to match the number of carbon, hydrogen and oxygen atoms on each side.
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This document provides information about chemical reactions and equations. It defines a chemical reaction as the transformation of reactants into products through the making or breaking of bonds. Examples of chemical reactions in daily life are given. A chemical equation represents reactants on the left side of an arrow and products on the right side. Balancing chemical equations ensures the number of each type of atom is equal on both sides, according to the law of conservation of mass. Steps for writing and balancing chemical equations are outlined with examples.
Balancing_Chemical_Equations.pptx
1) The document discusses balancing chemical equations, including identifying reactants and products, using subscripts and coefficients, and following the law of conservation of mass.
2) Balancing equations involves adjusting coefficients so that the same number and type of atoms are on both sides of the reaction arrow.
3) Examples show balancing equations by changing coefficients like N2 + H2 → 2NH3 and KClO3 → 2KCl + 3/2O2.
Chemical nomenclature and reactions
This document provides information about chemical nomenclature and reactions. It discusses writing chemical formulas, empirical formulas, chemical naming conventions, chemical equations, balancing equations, and types of chemical reactions. Specifically, it covers how to write formulas using oxidation numbers and valence, how to determine empirical and molecular formulas from composition data, rules for naming ionic and molecular compounds, the components and symbols used in chemical equations, and methods for balancing equations. It also defines four main types of chemical reactions: combination, decomposition, single displacement, and double displacement.
Balancing_Chemical_Equations.ppt
This document discusses chemical equations and balancing chemical reactions. It explains that a chemical equation describes a chemical change and is made up of reactants on the left and products on the right, with coefficients showing quantities. Balancing equations involves adjusting these coefficients to satisfy the law of conservation of mass, ensuring the same number and type of atoms enter and leave the reaction. Several examples of balancing equations are provided.
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- 3. REACTANTS: SUBSTANCE THAT INTERACTS WITH ONE ANOTHER IN A CHEMICAL REACTION, THEY ARE WRITTEN ON THE LEFT SIDE OF A CHEMICAL EQUATION. PRODUCTS: SUBSTANCE FORMED BY A CHEMICAL REACTION, THEY ARE WRITTEN ON THE RIGHT SIDE OF A CHEMICAL EQUATION.
- 5. " " COMMON SYMBOLS .
- 6. These guidelines are summarized as follows: Guidelines #1- write the correct formula Guideline #2-start with a specific element in a compound with the most atoms. Guidelines#3 –balance the polyatomic ions. Guidelines#4-balance the H atoms and then O atoms . Guideline#5- checks the coefficients to see that they are whole numbers and are in the lowest possible ratio. Guideline#6- check off each atom or polyatomic ion with a check.
- 7. EXAMPLE: 1. H2SO4 + CA(OH)2 CASO4 + H2O H2SO4 + CA(OH)2 CASO4 + 2H2O