Lesson 13 and 14
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This 2 page Class Notes was uploaded by Kara Nichols on Tuesday June 21, 2016. The Class Notes belongs to CHM 111 at Calhoun Community College taught by Mona Chaudhary in Spring 2016. Since its upload, it has received 15 views.
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Date Created: 06/21/16
Lesson 13 ● Balancing chemical equations ○Reactants -> Products ○Conservation of matter: matter cannot be created nor destroyed ■ there must be the same number of molecules on each side ■ H + OH -2H ● 2 hydrogen on the left, 2 hydrogen on the right ● 1 oxygen on the left, 1 oxygen on the right ○To balance chemical equations: ■ balance all molecules except Oxygen and Hydrogen ● Balance Hydrogen next ● then, balance Oxygen ■ Do not change subscripts (the small numbers) ■ only change the coefficients (the numbers in front) ● Chemical equations are ratios ○moles:moles ○molecules:molecules ○mass:mass ○Before you can do any calculations, the chemical equation must be balanced Lesson 14 ● Limiting Reactants ○the limiting reactant stops the reaction when it is used up ■ if you have 3 slices of bread, and 2 slices of cheese, how many sandwiches can you make? ■ 1, because you only have enough bread to make 1 sandwich ○The amount of product that is created depends on the limiting reactant ○Start witalancreaction, then use the fencing method to solve (shown below) ● Solve a problem: ○Balance the equation ○treat each reaction as if it were the limiting reactant ○the reactant that has the smallest number of product will be the limiting reactant ■the reactant with the large amount of product will be the excess reactant ○ Given the unbalanced equation: ■N2 4 N2 4 N2+ H2 ■what mass (g)2ould be produced by the reaction of 850g of N2 4d 550g2 4 ■What is the limiting reactant? ■What is the excess reactant? ■How much of the excess reactant is left over? ■What is the theoretical yield? ■Of the reaction actually produc2what is the percent yield for the reaction?
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