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Chemical Equations and Stoichiometry

Chemical Equations and Stoichiometry. Chapter 4. Chemical Equations. 2H 2 (g) + O 2 (g) ? 2H 2 O(g). Chemical Equations. 2H 2 (g) + O 2 (g) ? 2H 2 O(g) The materials you start with are called Reactants . Chemical Equations. 2H 2 (g) + O 2 (g) ? 2H 2 O(g)

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Chapter 15

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Sodium hydroxide and hydrobromic acid

Sodium hydroxide and hydrobromic acid. NaOH (aq) +HBr (aq) ?NaBr (aq) +H 2 O (l). OH - (aq) +H + (aq) ?H 2 O (l). Propane combusts. 2C 4 H 10(g) +O 2(g) ?8CO 2(g) + 10H 2 O (l). 2C 4 H 10(g) +O 2(g) ?8CO 2(g) + 10H 2 O (l). Potassium and water. 2K (s) +2H 2 0 (l) ?2KOH (aq) +H 2(g).

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Energy

Energy. The capacity to do work or to produce heat. System and Surroundings. System : That on which we focus attention Surroundings : Everything else in the universe Universe = System + Surroundings. Figure 6.9. Components of internal energy (E). Components of Internal Energy.

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Special Note: Endothermic Reactions

Special Note: Endothermic Reactions. As long as the total entropy is slightly positive, endothermic reactions will go forward Spontaneity is determined by the increase in the entropy of the system, NOT a decrease in the ENERGY (heat) of the system!. ?. Equilibrium.

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Energetics

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Equilibrium Systems and Stress

Equilibrium Systems and Stress . Chemical Equilibrium. Chemical Equilibrium When the rates of the forward and reverse reactions are equal in a chemical reaction The concentration (amount) of reactants and products of the reaction remains the same Ex: 2CO (g) + O 2(g) ? 2O 2(g).

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Chemical Kinetics

Chemical Kinetics. CA Standards. Collision Model. Collisions must have enough energy to produce the reaction (must equal or exceed the activation energy). Reactants must have proper orientation to allow the formation of new bonds. Activation Energy.

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2.0 0.5 0.20 5.0 0.012

For the reaction 2A + B {image} C + 2D at 35°C, the value of kf is 3.0 x 10-3 M-2•s-1 and the value of kr = 1.5 x 10-2 M-2•s-1. Calculate the value of Kc for this reaction. 2.0 0.5 0.20 5.0 0.012.

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Information given by chemical equations

Information given by chemical equations. 2 C 6 H 6 (l) + 15 O 2 (g) ? 12 CO 2 (g) + 6 H 2 O (g). In this equation there are 2 molecules of benzene reacting with 15 molecules of oxygen to produce 12 molecules of carbon dioxide and 6 molecules of water .

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WRITING CHEMICAL EQUATIONS

WRITING CHEMICAL EQUATIONS. Reactants (starting materials) ? Products (ending materials) (g) = gas (l) = liquid (s) = solid (aq) = aqueous D = heat ? = yields (dissolved in water) X ? = catalyst + = combines

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Increasing energy with temp?

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Hess's Law

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Reaction Types

Reaction Types. Combination (Synthesis) Reactions. Two or more substances combine to form a new compound. A + X ? AX. Reaction of elements with oxygen and sulfur Reactions of metals with Halogens Synthesis Reactions with Oxides There are others not covered here!.

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Hess's Law

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Which of the following reactions could be classified as exothermic ?

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Types of Chemical Reactions

Types of Chemical Reactions. Combination/Synthesis Reaction. General Equation: R + S ? RS Reactants: Generally two elements or two compounds. Probable Products: A single compound Example: 2Mg (s) + O 2(g) ? 2MgO (s ) Practice problems pg 214 #13-14. Decomposition. General Equation:

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Blast Furnace Reactions

Blast Furnace Reactions. Carbon oxidised by hot air:. Carbon (s) + oxygen (g) ? carbon dioxide (g). C (s) + O 2 (g) ? C O 2 (g). Carbon oxidised by carbon dioxide:. Carbon (s) + carbon dioxide (g) ? carbon monoxide (g). C (s) + CO 2 (g) ? 2C O (g).

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