Chapter Eighteen Energy and Reactions 18 1 Energy

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Chapter Eighteen: Energy and Reactions Ø 18. 1 Energy and Chemical Reactions Ø 18.

Chapter Eighteen: Energy and Reactions Ø 18. 1 Energy and Chemical Reactions Ø 18. 2 Chemical Reaction Systems Ø 18. 3 Nuclear Reactions

18. 2 Chemical Reaction Systems ØA balanced chemical equation is like a recipe. ØIf

18. 2 Chemical Reaction Systems ØA balanced chemical equation is like a recipe. ØIf you write the equation for making chocolate cake, you will see it is similar to a real recipe for making water.

18. 2 Chemical Reaction Systems

18. 2 Chemical Reaction Systems

18. 2 Information from Balanced Chemical Equations ØIf the recipe for chocolate cake gives

18. 2 Information from Balanced Chemical Equations ØIf the recipe for chocolate cake gives you ratios among the ingredients needed to make eight servings, how many servings are possible if you only have half a cup of flour?

18. 2 Information from Balanced Chemical Equations ØTo make a good-tasting chocolate cake with

18. 2 Information from Balanced Chemical Equations ØTo make a good-tasting chocolate cake with half as much flour, you would have to use half as much of the other ingredients, too. ØBy halving the recipe, you can make four servings of chocolate cake.

18. 2 Information from Balanced Chemical Equations ØA balanced chemical equation shows the ratios

18. 2 Information from Balanced Chemical Equations ØA balanced chemical equation shows the ratios of the number of molecules of reactants needed to make a certain number of molecules of products using coefficients.

18. 2 What a balanced equation doesn’t tell you ØA balanced equation does not

18. 2 What a balanced equation doesn’t tell you ØA balanced equation does not describe the exact conditions under which a reaction will occur. ØThe right conditions for most of the reactions that are used in science and industry are the result of careful research and experimentation.

18. 2 Limiting and Excess Reactants ØWhen a chemical reaction occurs, the reactants are

18. 2 Limiting and Excess Reactants ØWhen a chemical reaction occurs, the reactants are not always present in the exact ratio indicated by the balanced equation. ØWhat usually happens is that a chemical reaction will run until the reactant that is in short supply is used up.

18. 2 Limiting and Excess Reactants ØThe reactant that is used up first in

18. 2 Limiting and Excess Reactants ØThe reactant that is used up first in a chemical reaction is called the limiting reactant. ØThe limiting reactant limits the amount of product that can be formed. Which reactant will be used up first?

18. 2 Limiting and Excess Reactants ØA reactant that is not completely used up

18. 2 Limiting and Excess Reactants ØA reactant that is not completely used up is called an excess reactant because some of it will be left over when the reaction is complete. Which reactant will be left over (mixed with) product?

18. 2 Percent Yield Ø Often the amount of product you are able to

18. 2 Percent Yield Ø Often the amount of product you are able to collect and measure is less than the amount you would expect. Ø Experimental error often affects how much product is produced.

18. 2 Percent Yield Ø The percent yield (%) is the actual yield divided

18. 2 Percent Yield Ø The percent yield (%) is the actual yield divided by the predicted yield and then multiplied by one hundred.

Solving Problems ØAspirin can be made in the laboratory through a series of reactions.

Solving Problems ØAspirin can be made in the laboratory through a series of reactions. ØIf the actual yield for aspirin was 461. 5 grams when the reactions were performed, and the predicted yield was 500 grams, what was the percent yield?

Solving Problems 1. Looking for: Ø …percent yield of reaction 2. Given Ø Actual

Solving Problems 1. Looking for: Ø …percent yield of reaction 2. Given Ø Actual yield = 461. 5 g Ø Predicted yield = 500. 0 g 3. Relationships: Ø percent yield = actual yield predicted yield 4. Solution × 100% Ø percent yield = (461. 5 g ÷ 500. 0 g) × 100 = 92. 3%

18. 2 Reaction Rates ØIn all phases of matter, atoms and molecules exhibit random

18. 2 Reaction Rates ØIn all phases of matter, atoms and molecules exhibit random motion. ØThis concept is part of the kinetic theory of matter. ØThe speed at which atoms or molecules move depends on the state of matter and temperature.

18. 2 Reaction Rates Ø The reaction rate for a chemical reaction is the

18. 2 Reaction Rates Ø The reaction rate for a chemical reaction is the change in concentration of reactants or products over time. Ø Reaction rates can be increased by: 1. adding heat to increase molecular motion 2. increasing the concentration of the reactants 3. increasing the chances that two molecules will collide.

18. 2 Catalysts Ø A catalyst is a molecule that can be added to

18. 2 Catalysts Ø A catalyst is a molecule that can be added to a reaction to speed it up. Ø Catalysts work by increasing the chances that two molecules will be positioned in the right way for a reaction to occur.

18. 2 Chemical equilibrium ØA reaction may reach chemical equilibrium, the state in which

18. 2 Chemical equilibrium ØA reaction may reach chemical equilibrium, the state in which the rate of the forward reaction equals the rate of the reverse reaction. ØIn chemical equilibrium, the reaction can proceed both left and right simultaneously.

18. 2 Chemical vs. Nuclear Reactions ØFor complex reasons, the nucleus of an atom

18. 2 Chemical vs. Nuclear Reactions ØFor complex reasons, the nucleus of an atom becomes unstable if it contains too many or too few neutrons relative to the number of protons. ØThe forces inside the atom result in it breaking apart or releasing particles.

Radioactive Decay ØThis process of radioactive decay results in an unstable, radioactive isotope like

Radioactive Decay ØThis process of radioactive decay results in an unstable, radioactive isotope like carbon 14 becoming the more stable isotope nitrogen-14.

Radioactive Decay Ø There are three types of radioactive decay: 1. alpha decay, 2.

Radioactive Decay Ø There are three types of radioactive decay: 1. alpha decay, 2. beta decay, and 3. gamma decay.

Two types of Nuclear Reactions ØThere are two kinds of nuclear reactions: fusion and

Two types of Nuclear Reactions ØThere are two kinds of nuclear reactions: fusion and fission. Ø Nuclear fusion is the process of combining the nuclei of lighter atoms to make heavier atoms.