Balancing Equations Worksheet 1) ____ Na3PO4 + ____ KOH ( ____ NaOH + ____ K3PO4 2) ____ MgF2 + ____ Li2CO3 ( ____ MgCO3 + ____ LiF 3) ____ P4 + ____ O2 ( ____ P2O3 4) ____ RbNO3 + ____ BeF2 ( ____ Be(NO3)2 + ____ RbF 5) ____ AgNO3 + ____ Cu ( ____ Cu(NO3)2 + ____ Ag 6) ____ CF4 + ____ Br2 ( ____ CBr4 + ____ F2 7) ____ HCN + ____ CuSO4 ( ____ H2SO4 + ____ Cu(CN)2 8) ____ GaF3 + ____ Cs ( ____ CsF + ____ Ga 9) ____ BaS + ____ PtF2 ( ____ BaF2 + ____ PtS 10) ____ N2 + ____ H2 ( ____ NH3
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09. Net Ionic Equations tutorial.doc Introduction to Net Ionic Equations This tutorial will give you an algorithm for writing net ionic equations for aqueous reactions in general chemistry. Knowledge of the solubility rules is necessary to complete this tutorial. A list of solubility rules is provided at the end of the tutorial for review. Net ionic equations are necessary in chemistry for several reasons: 1. They show only those species undergoing chemical change – “spectator” ions are removed
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Single Replacement Reactions a. For every reaction that took place you must write the balanced chemical equation b. Which metal reacted the most? c. Rank your metals from more to least active Part II: Double replacement Reactions a. For every reaction where you observed precipitate, write the complete balanced molecular equation, the complete ionic equation and the net ionic equation; use the solubility rules to identify the precipitate and the states of matter of each substance
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calculators (non-programmable and non-graphing) are allowed to be with students during exams. Students are not allowed to take an exam in a lecture section in which they are not registered. Chapter 4 – sections 4.1 – 4.8 Given a balanced chemical equation, you should be able to calculate grams (or moles) of a product (or reactant) given the grams (or moles) of another product (or reactant). Remember: grams A ( moles A ( moles B ( grams B (p. 118). Practice Example 4.1
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Oxidation-reduction reactions (or redox) reactions, are a type of reaction in aqueous solutions that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an e-. They occur every day and are vital to some of the basic functions of life. Some examples include photosynthesis (within plants), respiration (within animals), combustion, and corrosion or rusting
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Bryan Ralloma Jennifer Caraway CHEM 1405-034 April 9, 2014 Balancing and Classifying Synthesized Chemical Reactions Abstract During the experimentation, physical and chemical properties of unaltered elements/compounds were noted. The alteration of these physical and chemical properties, were understood to have defined chemical change. The experimental procedures were divided into five phases: Magnesium and Oxygen, Zinc and Copper(II) Sulfate, Metals and HCl, Reactions of Ionic Compounds, and
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| | | 1. Part 2: Single-Displacement Reactions: For each four single-displacement reaction, describe what happened in each well. If a chemical reaction occurred, write a balanced equation for it. Then use the A, B symbols to write a general equation for a single-displacement reaction. Here are the chemical formulas of the reactants for each reaction: • zinc – Zn copper sulfate – CuSO4 • aluminum – Al copper sulfate – CuSO4 • zinc – Zn
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number – 6.022 x 10^23 * How to determine how many atoms of each element is in a compound: * (moles or grams)(6.022x10^23)(Number of atoms/1molecule) * Molar mass - Molar mass is the weight of one mole (or 6.022 x 1023 molecules) of any chemical compounds. * Mass % of an element in a compound: * ((Number of atoms of element)(atomic weight))/(Formula weight) * Empirical formula – Gives the lowest whole number ratio of atoms of each element in a compound (Grams)/(atomic weight)
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CHAPTER 3 MASS RELATIONSHIPS IN CHEMICAL REACTIONS This chapter reviews the mole concept, balancing chemical equations, and stoichiometry. The topics covered in this chapter are: • Atomic mass and average atomic mass • A vogadro’ s number, mole, and molar mass • Percent composition calculations • Empirical and molecular formula determinations • Chemical equations, amount of reactant and product calculations • Limiting reagents and reaction yield calculations Take Note: It is absolutely essential
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Stoichiometry is simply the math behind chemistry. Given enough information, one can use stoichiometry to calculate masses, moles, and percents within a chemical equation. ________________________________________ ________________________________________ What is a Chemical Equation? In chemistry, we use symbols to represent the various chemicals. Success in chemistry depends upon developing a strong familiarity with these basic symbols. For example, the symbol "C"represents an atom of carbon, and
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