In order to use this relationship, however, we must use the molar mass of to convert grams of to moles of Because 1 mol we have The coefficients in Equation 3.12 tell how the amount of consumed is related to the amount of produced: 2 mol Let's calculate the mass of produced when 1.00 g of is burned. ( ), the fuel in disposable cigarette lighters: For example, the number of moles of produced from 1.57 mol of can be calculated as follows:Īs an additional example, consider the combustion of butane Where the symbol means "stoichiometrically equivalent to." In other words, Equation 3.11 shows 2 mol ofĪnd 1 mol of forming 2 mol of These stoichiometric relations can be used to convert between quantities of reactants and products in a chemical reaction. The relationship between these quantities can be represented The quantities 2 mol 1 mol and 2 mol which are given by the coefficients in Equation 3.11, are called stoichiometrically equivalent quantities. Involved in the reaction and as the relative numbers of moles. The coefficients in a balanced chemical equationĬan be interpreted both as the relative numbers of molecules (or formula units)
The coefficients tell us that two molecules of react with each molecule of to form two molecules of It follows that the relative numbers of moles are identical to the relative numbers of molecules: Consider the following balanced equation: The mole concept allows us to use the quantitative information available in a balanced equation on a practical macroscopic level.