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CHM2045 Lecture Notes - Lecture 3: Molar Mass, Limiting Reagent, Molecular Mass

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turquoiseserval308

9 Feb 2020

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Predict the products of simple combination, decomposition, and combustion reactions. Convert grams to moles and moles to grams using molar masses. Convert number of molecules to moles and moles to number of molecules using. Calculate the empirical and molecular formulas of a compound from percentage composition and molecular weight. Identify limiting reactants and calculate amounts, in grams or moles, or reactants consumed and products formed for a reaction. Stoichiometry is the study of the quantitative relationships in substances and their reactions. Chemical equations: a chemical equation is a shorthand notation to describe a chemical reaction. Just like a chemical formula, a chemical equation expresses quantitative relations: subscripts tell the number of atoms of each element in a molecule, coefficients tell the number of molecules. Hydrogen and oxygen can make water or hydrogen peroxide. Reactants appear on the left side of the equation. Products appear on the right side of the equation.

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Related Questions

To understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. Stoichiometry describes the quantitative relationships among the reactants and products of a balanced reaction by directly comparing mole ratios. Stoichiometry can be used to convert mass, number of moles, or number of partides between products and reactants, as shown in the flowchart displayed in the figure. (Figure 1) How many grams of NH3 can be produced from 2.21molofN2 and excess HÂ« Express your answer numerically in grams. How many grams of H2 3re needed to produce 10.14g of NH3 ? Express your answer numerically in grams. How many molecules {not moles) of NHa are produced from 8.42 times 10-1g of Hg? Express your answer numerically as the number of molecules. In the following chemical reaction 2 mol of A will react with 1 mol of B to produce 1 mol of A B without anything left over: But what if you re given 2.8 mol of A and 3.2 mol of B7 The amount of product formed is limited by the reactant that runs out first, called the limiting reactant. To identify the limiting reactant, calculate the amount of product formed from each amount of reactant separately: Notice that less product is formed with the given amount of reactant A. Thus. A is the limiting reactant, and a maximum of 1.4 mol of A2B can be formed from the given amounts. If you had excess chlorine, how many moles of of aluminum chloride could be produced from 11 .Og of aluminum'7 Express your answer to three significant figures and include the appropriate units. Part B If you had excess aluminum, how many moles of aluminum chloride could be produced from 16.0g of chlorine gas, Limiting Reactant Procedure Express your answer to three significant figures and include the appropriate units. Part C Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: What is the maximum mass of aluminum chloride that can be formed when reacting 11.0g of aluminum with 16.3g of chlorine17 Express your answer to three significant figures and include the appropriate units.

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