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180 Chapter 4 Stoichiometry of Chemical Reactions It is sometimes convenient to use fractions instead of integers as intermediate coefficients in the process of balancing a chemical equation. When balance is achieved, all the equation’s coefficients may then be multiplied by a whole number to convert the fractional coefficients to integers without upsetting the atom balance. For example, consider the reaction of ethane (C2H6) with oxygen to yield H2O and CO2, represented by the unbalanced equation: C2H6+O2 ⟶H2O+CO2 (unbalanced) Following the usual inspection approach, one might first balance C and H atoms by changing the coefficients for the two product species, as shown: C2H6+O2 ⟶3H2O+2CO2 (unbalanced) This results in seven O atoms on the product side of the equation, an odd number—no integer coefficient can be used with the O2 reactant to yield an odd number, so a fractional coefficient, 72, is used instead to yield a provisional balanced equation: C2H6+ 72O2 ⟶3H2O+2CO2 A conventional balanced equation with integer-only coefficients is derived by multiplying each coefficient by 2: 2C2H6 +7O2 ⟶ 6H2O+4CO2 Finally with regard to balanced equations, recall that convention dictates use of the smallest whole-number coefficients. Although the equation for the reaction between molecular nitrogen and molecular hydrogen to produce ammonia is, indeed, balanced, 3N2+9H2 ⟶6NH3 the coefficients are not the smallest possible integers representing the relative numbers of reactant and product molecules. Dividing each coefficient by the greatest common factor, 3, gives the preferred equation: N2+3H2 ⟶2NH3 Link to Learning Use this interactive tutorial (http://openstaxcollege.org/l/16BalanceEq) for additional practice balancing equations. Additional Information in Chemical Equations The physical states of reactants and products in chemical equations very often are indicated with a parenthetical abbreviation following the formulas. Common abbreviations include s for solids, l for liquids, g for gases, and aq for substances dissolved in water (aqueous solutions, as introduced in the preceding chapter). These notations are illustrated in the example equation here: 2Na(s) + 2H2 O(l) ⟶ 2NaOH(aq) + H2(g) This equation represents the reaction that takes place when sodium metal is placed in water. The solid sodium reacts with liquid water to produce molecular hydrogen gas and the ionic compound sodium hydroxide (a solid in pure form, but readily dissolved in water). This content is available for free at http://cnx.org/content/col11760/1.9PDF Image | Stoichiometry of Chemical Reactions
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