The answer could also be written in other, equally valid ways:
Balancing a Chemical Equation . Balance this equation for the combustion of butane, the fluid most commonly used in pocket lighters:Strategy : The equation for the combustion of butane is very similar to the one we examined at the beginning of this section for the combustion of propane. To
Stoichiometry . When urea, (NH)2 2CO, is acted on by the enzyme urease in the presence of water, ammonia and carbon dioxide are produced. Urease, the catalyst, is placed over the reaction arrow.If excess water is present (more than necessary for the reaction), how many grams each of CO2 and NH3
Stoichiometry . Silicon to be used in computer chips is manufactured by a process represented by the following reaction:A sample of 225 g of silicon tetrachloride, SiCl4, is reacted with an excess (more than necessary) of Mg. How many moles of Si are produced? Strategy : To solve this example,
Stoichiometry . Ammonia is produced on an industrial scale by the reaction of nitrogen gas with hydrogen gas (the Haber process) according to this balanced equation: How many grams of N2 are necessary to produce 7.50 g of NH3?
Balancing a Chemical Equation . Balance this equation:
Oxidation–Reduction . In each equation, identify the substance that is oxidized, the substance that is reduced, the oxidizing agent, and the reducing agent.
Net Ionic Equation .Of the four ways for ions to react in water, one of the most common is the formation of an insoluble compound. We can predict when this result will happen if we know the solubilities of the ionic compounds. Some useful guidelines for the solubility of ionic compounds in water
Percent Yield . In an experiment forming ethanol, the theoretical yield is 50.5 g. The actual yield is 46.8 g. What is the percent yield?Strategy: Percent yield is the actual yield divided by the theoretical yield times 100
Limiting Reagent . Suppose 12 g of C is mixed with 64 g of O2, and the following reaction takes place: C(s) + O2 (g)→ CO2 (g2) (a) Which reactant is the limiting reagent and which reactant is in excess?(b) How many grams of CO2 will be formed? Strategy : Determine how many moles of each reactant