![]() during a molar volume of oxygen experiment indicate how each of the following errors would affect (increase, decrease, or no change) your calculated value for the molar volume of O2 at STP.ġ.) Your sample was not completely decomposed.calculate the molar volume (volume of 1.0 mole) of an ideal gas at 1.0 atm and 25 degrees celsius.The molar heat of reaction, H rxn, for the reaction ofĬa(s) + 2H+(aq)-> Ca2+(aq) + H2(g) was found to be -550kJ/mol The change Hrxn, for the reaction of CaO(s) + 2H+(aq)-> Ca2+(aq) + H2O(l) was found to be -189kJ/mol Based on these results if the.How long will it take an identical balloon filled with the same number of moles of air (ℳ = 28.2 g/mol) to deflate to 1/2 of its original volume? A party balloon filled with helium deflates to 2/3 of its original volume in 8.0 hours.(Dimers are molecules formed from the combination of identical molecules, A + A -> A2.) What effect would this have on the experimental molar mass? Some liquids have enough attractions between molecules to form dimers.Volume (dm3) of acid needed to prepare 2.00 dm3 of 3.00 mol dm-3 HNO3 solution. The density of 19.0% by mass of nitric acid, HNO3 is 1.11 g cm-3.27) What volume of benzene (C6H6, d= 0.88 g/mL, molar mass = 78.11 g/mol) is required to produce 1.5 x 103 kJ of heat according to the following reaction? Textbook content produced by OpenStax is licensed under a Creative Commons Attribution License. We recommend using aĪuthors: Paul Flowers, Klaus Theopold, Richard Langley, William R. Use the information below to generate a citation. ![]() Then you must include on every digital page view the following attribution: If you are redistributing all or part of this book in a digital format, Then you must include on every physical page the following attribution: If you are redistributing all or part of this book in a print format, Want to cite, share, or modify this book? This book uses the If the molecular (or molar) mass of the substance is known, it may be divided by the empirical formula mass to yield the number of empirical formula units per molecule ( n): As the name suggests, an empirical formula mass is the sum of the average atomic masses of all the atoms represented in an empirical formula. Molecular formulas are derived by comparing the compound’s molecular or molar mass to its empirical formula mass. Molar mass can be measured by a number of experimental methods, many of which will be introduced in later chapters of this text. Molecular mass, for example, is often derived from the mass spectrum of the compound (see discussion of this technique in the previous chapter on atoms and molecules). These quantities may be determined experimentally by various measurement techniques. Determining the absolute numbers of atoms that compose a single molecule of a covalent compound requires knowledge of both its empirical formula and its molecular mass or molar mass. Recall that empirical formulas are symbols representing the relative numbers of a compound’s elements. The percent composition of this compound could be represented as follows: For example, consider a gaseous compound composed solely of carbon and hydrogen. The results of these measurements permit the calculation of the compound’s percent composition, defined as the percentage by mass of each element in the compound. When a compound’s formula is unknown, measuring the mass of each of its constituent elements is often the first step in the process of determining the formula experimentally. The elemental makeup of a compound defines its chemical identity, and chemical formulas are the most succinct way of representing this elemental makeup. ![]() But what if the chemical formula of a substance is unknown? In this section, these same principles will be applied to derive the chemical formulas of unknown substances from experimental mass measurements. Given the chemical formula of the substance, one may determine the amount of the substance (moles) from its mass, and vice versa. The previous section discussed the relationship between the bulk mass of a substance and the number of atoms or molecules it contains (moles). ![]() Determine the molecular formula of a compound.Determine the empirical formula of a compound.Compute the percent composition of a compound.By the end of this section, you will be able to: ![]()
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