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This document provides an introduction to chemical reactions. It explains that chemical reactions are represented by chemical equations that show the same number of atoms of each element on both sides. Some examples of chemical reactions mentioned include cooking, respiration, hair dye, and auto fuel. The document also discusses how chemists observe reactions and represent them with chemical equations. It provides an example chemical equation for making NaCl. Additionally, it explains the differences between chemical and numerical equations and the symbols used in chemical equations like state symbols. Finally, it discusses how to balance chemical equations by making sure the same number of atoms of each element are on both sides of the equation.
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Balancing Chemical Equations 1
A chemical equation represents a chemical reaction, showing the reactants on the left and products on the right separated by an arrow. For the equation to be balanced, the number of atoms of each type must be equal on both sides. To balance an equation, you take an atom inventory, split the equation into reactants and products, then add coefficients in front of the chemical formulas to make the number of atoms equal on both sides.
Balancing chemical equations notes
This document discusses balancing chemical equations. It explains that a chemical equation uses symbols and formulas to represent a chemical reaction and must obey the law of conservation of mass. This law states that the number and type of atoms on the reactants side must equal the number and type on the products side. The document shows an example of an unbalanced equation and uses coefficients to balance the atoms, resulting in an equation that follows the law of conservation of mass.
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This document discusses chemical equations and reactions. It explains that chemical equations are used to represent chemical reactions, and that they consist of reactants on the left side of the arrow yielding products on the right. It also describes how to balance chemical equations by adjusting coefficients so that the same number of each type of atom is on both sides of the equation. Balancing chemical equations ensures conservation of mass during chemical reactions.
Balancing Chemical Equations
1) A chemical equation is a symbolic representation of a chemical reaction using element symbols and formulas to show reactants and products.
2) Chemical equations must be balanced so that the same number of each type of atom is on both sides of the reaction arrow.
3) To balance equations, coefficients are placed in front of formulas to adjust the relative numbers of elements and compounds until both sides have equal quantities.
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The document discusses chemical equations and balancing chemical reactions. It explains that a chemical equation uses symbols to show the reactants on the left and products on the right, with an arrow indicating the direction of the reaction. It also discusses the law of conservation of mass, which states that the total mass and number of atoms is conserved in chemical reactions. Balancing chemical equations ensures the number of atoms of each element is the same on both sides of the reaction. Adding state symbols provides additional information about the phases of the substances involved.
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The document discusses physical and chemical changes in matter. A physical change alters the form of matter but not its identity, and can be reversed. A chemical change produces new substances through chemical reactions, with the mass and number of atoms conserved but molecules changing. Chemical changes involve more energy and are not easily reversible. The document also outlines laws of conservation of mass and constant composition, and Gay-Lussac's law regarding gas reactions.
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This document provides instructions for balancing chemical equations. It explains that chemical equations must be balanced to show the same number of atoms of each element on both sides. The steps provided to balance an equation are to: draw boxes around formulas, make an element inventory, and add coefficients to formulas until the inventory is equal on both sides, showing the reaction is balanced. An example reaction and balancing steps are shown. Key aspects are to never change what is in the boxes, keep the inventory updated, and simplify coefficients if possible.
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This document discusses balancing chemical equations. It explains that a chemical equation uses symbols and formulas to represent a chemical reaction and must obey the law of conservation of mass. This law states that the number and type of atoms on the reactants side must equal the number and type on the products side. The document shows an example of an unbalanced equation and uses coefficients to balance the atoms, resulting in an equation that follows the law of conservation of mass.
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2. Rules for balancing equations include writing unbalanced formulas with an arrow between reactants and products, counting atoms on each side, and balancing one element at a time using the lowest common multiple as the coefficient.
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Fundament
als of
Chemistry
Module 2 – Chapter 8
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forming.
• Indicate specific amounts of materials consumed or produced during the
reaction.
• Reactants: substances consumed during the reaction.
• Products: substances formed during the reaction.
• Atom balance must be maintained in all chemical reactions.
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a A + b B c C + d D
The
coefficient
1 is not
written in
a balanced
equation.
Chemical Equations
1. Reactants and products are separated by an arrow.
2. Reactants are on the left side of the arrow, products are on the right.
3. Whole number coefficients are placed in front of substances to
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during the reaction.
5. Information about the reaction (temperature, time) may be placed
above or below the reaction arrow.
6. The physical state is written in brackets after the formula of the
substance. (g) for gas, (l) for liquid, (s) for solid, (aq) for aqueous
a A + b B c C + d D
Reactant
s
Products
Symbol
Summary
Symbol Significance
Produces (points towards products)
(s) Solid (written after substance)
(l) Liquid (written after substance)
(g) Gas (written after substance)
(aq) Substance dissolved in an aqueous
solution
Heat is added (above or below reaction
arrow)
Δ
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Δ
Hg: 1
O: 1
Hg: 1
O: 2
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Hg: 1
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This document discusses aqueous chemistry and chemical equilibrium. It introduces key concepts like the equilibrium constant K, reaction quotient Q, and Le Châtelier’s principle. K is a ratio that quantifies concentrations at equilibrium. Q is similar but used to predict the direction of reactions not yet at equilibrium. Le Châtelier's principle states that if a system at equilibrium experiences a change, it will shift to counteract the change.
notes-chemicalequations-131017003253-phpapp01.pptx
The document discusses chemical equations and balancing chemical reactions. It explains that a chemical equation uses symbols to represent chemical reactions and must follow the law of conservation of mass, which states that the number and type of atoms on both sides of a chemical reaction must be equal. Balancing chemical equations involves adding coefficients to reactants and products so the number of each type of atom is the same on both sides of the reaction.
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This document discusses chemical reactions and different types of reactions. It begins by defining a chemical reaction as a process where the atoms in reactants are rearranged to form new substances known as products. It describes the key components of a chemical reaction as reactants, products, and activation energy. It then provides examples of the six main types of chemical reactions: synthesis, combustion, decomposition, single displacement, double displacement, and acid-base reactions. It explains the basic mechanisms and components of each type of reaction.
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Power point vishnu
- 2. Introduction to ChemicalIntroduction to Chemical ReactionsReactions SUBMITTED BYSUBMITTED BY V ISHNU.S.PILLAIV ISHNU.S.PILLAI PHYSICAL SCIENCEPHYSICAL SCIENCE
- 3. Main IdeasMain Ideas Chemical Reactions are represented byChemical Reactions are represented by Chemical Equations.Chemical Equations. Chemical Equations are balanced toChemical Equations are balanced to show the same number of atoms of eachshow the same number of atoms of each element on each side.element on each side.
- 4. Chemical Reactions areChemical Reactions are EverywhereEverywhere CookingCooking RespirationRespiration
- 5. Chemical Reactions areChemical Reactions are EverywhereEverywhere Hair DyeHair Dye Auto FuelAuto Fuel
- 6. Representing ChemicalRepresenting Chemical ReactionsReactions Chemists observe chemical reactions and have comeChemists observe chemical reactions and have come up with a way to represent or model what isup with a way to represent or model what is happening.happening. Making NaClMaking NaCl Solid Sodium combines with Chlorine gas to makeSolid Sodium combines with Chlorine gas to make solid Sodium Chloride:solid Sodium Chloride: 2Na (s) + Cl2 (g)2Na (s) + Cl2 (g) 2NaCl2NaCl
- 7. Chemical Equations are differentChemical Equations are different from Numerical Equationsfrom Numerical Equations Numerical Equation: 3x + 2y = 47Numerical Equation: 3x + 2y = 47 Chemical Equation 2Na + Cl2Chemical Equation 2Na + Cl2 2NaCl2NaCl ReactantA + Reactant BReactantA + Reactant B ProductProduct The reactants are used up in forming the productThe reactants are used up in forming the product The arrowThe arrow shows the direction of the reactionshows the direction of the reaction
- 8. Symbols used inSymbols used in Chemical EquationsChemical Equations Symbol Purpose + Separates more than one reactant or product Separates reactants from products. Indicates direction of reaction (s) Identifies a solid state (aq) Identifies that something is dissolved in water (l) Identifies liquid state (g) Identifies gaseous state
- 9. Balancing EquationsBalancing Equations After you write a chemical equation you have to balance it toAfter you write a chemical equation you have to balance it to make sure that the same number of atoms of each elementmake sure that the same number of atoms of each element are on each side.are on each side. How would you balance this equation?How would you balance this equation? Li + H2OLi + H2O H2 + LiOHH2 + LiOH
- 10. Steps to Balancing a Chemical EquationSteps to Balancing a Chemical Equation
- 11. Example ContinuedExample Continued Change the Coefficients to make the number ofChange the Coefficients to make the number of atoms of each element equalatoms of each element equal Balance the Hydrogens:Balance the Hydrogens: CH4 + O2CH4 + O2 CO2 +CO2 + 22 H2OH2O Balance the Oxygens:Balance the Oxygens: CH4 +CH4 + 22 O2O2 CO2CO2 ++ 22 H2OH2O