Chapter 4

Balance the following equations by inspection. (a) \(\mathrm{SO}_{3} \longrightarrow \mathrm{SO}_{2}+\mathrm{O}_{2}\) (b) \(\mathrm{Cl}_{2} \mathrm{O}_{7}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{HClO}_{4}\) (c) \(\mathrm{NO}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{HNO}_{3}+\mathrm{NO}\) (d) \(\mathrm{PCl}_{3}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{3} \mathrm{PO}_{3}+\mathrm{HCl}\)

Balance the following equations by inspection. (a) \(\mathrm{P}_{2} \mathrm{H}_{4} \longrightarrow \mathrm{PH}_{3}+\mathrm{P}_{4}\) (b) \(\mathrm{P}_{4}+\mathrm{Cl}_{2} \longrightarrow \mathrm{PCl}_{3}\) (c) \(\mathrm{FeCl}_{3}+\mathrm{H}_{2} \mathrm{S} \longrightarrow \mathrm{Fe}_{2} \mathrm{S}_{3}+\mathrm{HCl}\) (d) \(\mathrm{Mg}_{3} \mathrm{N}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}+\mathrm{NH}_{3}\)

Write balanced equations based on the information given. (a) solid magnesium + oxygen gas \(\longrightarrow\) solid magnesium oxide (b) nitrogen monoxide gas + oxygen gas \(\longrightarrow\) nitrogen dioxide gas (c) gaseous ethane(C \(_{2} \mathrm{H}_{6}\) ) + oxygen gas \(\longrightarrow\) carbon dioxide gas + liquid water (d) aqueous silver sulfate \(+\) aqueous barium iodide \(\longrightarrow\) solid barium sulfate + solid silver iodide

Write balanced equations based on the information given. (a) solid magnesium \(+\) nitrogen gas \(\longrightarrow\) solid magnesium nitride (b) solid potassium chlorate \(\longrightarrow\) solid potassium chloride + oxygen gas (c) solid sodium hydroxide \(+\) solid ammonium chloride \(\longrightarrow\) solid sodium chloride \(+\) gaseous ammonia \(+\) water vapor (d) solid sodium + liquid water \(\longrightarrow\) aqueous sodium hydroxide \(+\) hydrogen gas

Write balanced equations to represent the complete combustion of each of the following in excess oxygen: (a) butane, \(\mathrm{C}_{4} \mathrm{H}_{10} ;\) (b) isopropyl alcohol, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{3} ;\) (c) lactic acid, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}\)

Write balanced equations to represent the complete combustion of each of the following in excess oxygen: (a) propylene, \(\mathrm{C}_{3} \mathrm{H}_{6} ;\) (b) thiobenzoic acid, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COSH}\) (c) glycerol, \(\mathrm{CH}_{2}(\mathrm{OH}) \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH}\)

Write balanced equations to represent: (a) the decomposition, by heating, of solid ammonium nitrate to produce dinitrogen monoxide gas (laughing gas) and water vapor (b) the reaction of aqueous sodium carbonate with hydrochloric acid to produce water, carbon dioxide gas, and aqueous sodium chloride (c) the reaction of methane \(\left(\mathrm{CH}_{4}\right),\) ammonia, and oxygen gases to form gaseous hydrogen cyanide (HCN) and water vapor

Write balanced equations to represent: (a) the reaction of sulfur dioxide gas with oxygen gas to produce sulfur trioxide gas (one of the reactions involved in the industrial preparation of sulfuric acid) (b) the dissolving of limestone (calcium carbonate) in water containing dissolved carbon dioxide to produce calcium hydrogen carbonate (a reaction producing temporary hardness in groundwater) (c) the reaction of ammonia and nitrogen monoxide to form nitrogen gas and water vapor

A 3.104 g sample of an oxide of manganese contains 1.142 grams of oxygen. Write a balanced chemical equation for the reaction that produces the compound from \(\mathrm{Mn}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g})\)

Iron metal reacts with chlorine gas. How many grams of \(\mathrm{FeCl}_{3}\) are obtained when \(515 \mathrm{g} \mathrm{Cl}_{2}\) reacts with excess Fe? $$ 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{Cl}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{FeCl}_{3}(\mathrm{s}) $$

If \(46.3 \mathrm{g} \mathrm{PCl}_{3}\) is produced by the reaction $$ 6 \mathrm{Cl}_{2}(\mathrm{g})+\mathrm{P}_{4}(\mathrm{s}) \longrightarrow 4 \mathrm{PCl}_{3}(\mathrm{l}) $$ how many grams each of \(\mathrm{Cl}_{2}\) and \(\mathrm{P}_{4}\) are consumed?

A laboratory method of preparing \(\mathrm{O}_{2}(\mathrm{g})\) involves the decomposition of \(\mathrm{KClO}_{3}(\mathrm{s})\) $$ 2 \mathrm{KClO}_{3}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{KCl}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g}) $$ (a) How many moles of \(\mathrm{O}_{2}(\mathrm{g})\) can be produced by the decomposition of \(32.8 \mathrm{g} \mathrm{KClO}_{3} ?\) (b) How many grams of \(\mathrm{KClO}_{3}\) must decompose to produce \(50.0 \mathrm{g} \mathrm{O}_{2} ?\) (c) How many grams of KCl are formed, together with \(28.3 \mathrm{g} \mathrm{O}_{2},\) in the decomposition of \(\mathrm{KClO}_{3} ?\)

A commercial method of manufacturing hydrogen involves the reaction of iron and steam. $$ 3 \mathrm{Fe}(\mathrm{s})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \stackrel{\Delta}{\longrightarrow} \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{s})+4 \mathrm{H}_{2}(\mathrm{g}) $$ (a) How many grams of \(\mathrm{H}_{2}\) can be produced from \(42.7 \mathrm{g}\) Fe and an excess of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) (steam)? (b) How many grams of \(\mathrm{H}_{2} \mathrm{O}\) are consumed in the conversion of \(63.5 \mathrm{g}\) Fe to \(\mathrm{Fe}_{3} \mathrm{O}_{4} ?\) (c) If \(14.8 \mathrm{g} \mathrm{H}_{2}\) is produced, how many grams of \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) must also be produced?

The reaction of calcium hydride with water can be used to prepare small quantities of hydrogen gas, as is done to fill weather-observation balloons. \(\mathrm{CaH}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow\) $$ \mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{g}) \text { (not balanced) } $$ (a) How many grams of \(\mathrm{H}_{2}(\mathrm{g})\) result from the reaction of \(127 \mathrm{g} \mathrm{CaH}_{2}\) with an excess of water? (b) How many grams of water are consumed in the reaction of \(56.2 \mathrm{g} \mathrm{CaH}_{2} ?\) (c) What mass of \(\mathrm{CaH}_{2}(\mathrm{s})\) must react with an excess of water to produce \(8.12 \times 10^{24}\) molecules of \(\mathrm{H}_{2} ?\)

The reaction of potassium superoxide, \(\mathrm{KO}_{2}\), is used in life- support systems to replace \(\mathrm{CO}_{2}(\mathrm{g})\) in expired air with \(\mathrm{O}_{2}(\mathrm{g}) .\) The unbalanced chemical equation for the reaction is given below. $$\mathrm{KO}_{2}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g}) \longrightarrow \mathrm{K}_{2} \mathrm{CO}_{3}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g})$$ (a) How many moles of \(\mathrm{O}_{2}(\mathrm{g})\) are produced by the reaction of \(156 \mathrm{g} \mathrm{CO}_{2}(\mathrm{g})\) with excess \(\mathrm{KO}_{2}(\mathrm{s}) ?\) (b) How many grams of \(\mathrm{KO}_{2}(\mathrm{s})\) are consumed per \(100.0 \mathrm{g} \mathrm{CO}_{2}(\mathrm{g})\) removed from expired air? (c) How many \(\mathrm{O}_{2}\) molecules are produced per milligram of \(\mathrm{KO}_{2}\) consumed?

Iron ore is impure \(\mathrm{Fe}_{2} \mathrm{O}_{3} .\) When \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing \(938 \mathrm{kg}, 523 \mathrm{kg}\) of pure iron is obtained. What is the mass percent \(\mathrm{Fe}_{2} \mathrm{O}_{3},\) by mass, in the ore sample, assuming that none of the impurities contain Fe?

Solid silver oxide, \(\mathrm{Ag}_{2} \mathrm{O}(\mathrm{s}),\) decomposes at temperatures in excess of \(300^{\circ} \mathrm{C},\) yielding metallic silver and oxygen gas. A 3.13 g sample of impure silver oxide yields \(0.187 \mathrm{g} \mathrm{O}_{2}(\mathrm{g}) .\) What is the mass percent \(\mathrm{Ag}_{2} \mathrm{O}\) in the sample? Assume that \(\mathrm{Ag}_{2} \mathrm{O}(\mathrm{s})\) is the only source of \(\mathrm{O}_{2}(\mathrm{g}) .\) [Hint: Write a balanced equation for the reaction.]

The rocket boosters of the space shuttle Discovery, launched on July \(26,2005,\) used a fuel mixture containing primarily solid ammonium perchlorate, \(\mathrm{NH}_{4} \mathrm{ClO}_{4}(\mathrm{s}),\) and aluminum metal. The unbalanced chemical equation for the reaction is given below. \(\mathrm{Al}(\mathrm{s})+\mathrm{NH}_{4} \mathrm{ClO}_{4}(\mathrm{s}) \longrightarrow\) $$ \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s})+\mathrm{AlCl}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{N}_{2}(\mathrm{g}) $$ What is the minimum mass of \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) consumed, per kilogram of \(\mathrm{Al}\), by the reaction of \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) and Al?[Hint: Balance the elements in the order \(\mathrm{Cl}, \mathrm{H},\) \(\mathrm{O}, \mathrm{Al}, \mathrm{N} .\)]

Without per forming detailed calculations, which of the following yields the same mass of \(\mathrm{CO}_{2}(\mathrm{g})\) per gram of compound as does ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) when burned in excess oxygen? (a) \(\mathrm{H}_{2} \mathrm{CO}\); (b) \(\mathrm{HOCH}_{2} \mathrm{CH}_{2} \mathrm{OH} ;\) (c) \(\mathrm{HOCH}_{2} \mathrm{CHOHCH}_{2} \mathrm{OH}\) (d) \(\mathrm{CH}_{3} \mathrm{OCH}_{3} ;\) (e) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\)

What are the molarities of the following solutes when dissolved in water? (a) \(2.92 \mathrm{mol} \mathrm{CH}_{3} \mathrm{OH}\) in 7.16 L of solution (b) \(7.69 \mathrm{mmol} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) in \(50.00 \mathrm{mL}\) of solution (c) \(25.2 \mathrm{g} \mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}\) in \(275 \mathrm{mL}\) of solution

What are the molarities of the following solutes? (a) sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) if \(150.0 \mathrm{g}\) is dissolved per \(250.0 \mathrm{mL}\) of water solution (b) urea, \(\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2},\) if \(98.3 \mathrm{mg}\) of the \(97.9 \%\) pure solid is dissolved in \(5.00 \mathrm{mL}\) of aqueous solution (c) methanol, \(\mathrm{CH}_{3} \mathrm{OH},(d=0.792 \mathrm{g} / \mathrm{mL})\) if \(125.0 \mathrm{mL}\) is dissolved in enough water to make 15.0 L of solution

What are the molarities of the following solutes? (a) aspartic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{5} \mathrm{NO}_{4}\right)\) if \(0.405 \mathrm{g}\) is dissolved in enough water to make \(100.0 \mathrm{mL}\) of solution (b) acetone, \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O},(d=0.790 \mathrm{g} / \mathrm{mL})\) if \(35.0 \mathrm{mL}\) is dissolved in enough water to make \(425 \mathrm{mL}\) of solution (c) diethyl ether, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{O},\) if \(8.8 \mathrm{mg}\) is dissolved in enough water to make 3.00 L of solution

How much (a) glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},\) in grams, must be dissolved in water to produce \(75.0 \mathrm{mL}\) of \(0.350 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} ?\) (b) methanol, \(\mathrm{CH}_{3} \mathrm{OH} \quad(d=0.792 \mathrm{g} / \mathrm{mL}),\) in milli- liters, must be dissolved in water to produce 2.25 L of \(0.485 \mathrm{M} \mathrm{CH}_{3} \mathrm{OH} ?\)

How much (a) ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(d=0.789 \mathrm{g} / \mathrm{mL}),\) in liters, must be dissolved in water to produce \(200.0 \mathrm{L}\) of 1.65 \(\mathrm{M} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH} ?\) (b) concentrated hydrochloric acid solution \((36.0 \%\) HCl by mass; \(d=1.18 \mathrm{g} / \mathrm{mL}),\) in milliliters, is required to produce 12.0 L of 0.234 M HCl?

In many communities, water is fluoridated to prevent tooth decay. In the United States, for example, more than half of the population served by public water systems has access to water that is fluoridated at approximately \(1 \mathrm{mg} \mathrm{F}^{-}\) per liter. (a) What is the molarity of \(\mathrm{F}^{-}\) in water if it contains \(1.2 \mathrm{mg} \mathrm{F}^{-}\) per liter? (b) How many grams of solid KF should be added to a \(1.6 \times 10^{8}\) L water reservoir to give a fluoride concentration of \(1.2 \mathrm{mg} \mathrm{F}^{-}\) per liter?

Which of the following is a \(0.500 \mathrm{M} \mathrm{KCl}\) solution? (a) \(0.500 \mathrm{g} \mathrm{KCl} / \mathrm{mL}\) solution; (b) \(36.0 \mathrm{g} \mathrm{KCl} / \mathrm{L}\) solu- tion; (c) 7.46 mg KCl/mL solution; (d) 373 g KCl in 10.00 L solution

Which has the higher concentration of sucrose: a \(46 \%\) sucrose solution by mass \((d=1.21 \mathrm{g} / \mathrm{mL}),\) or \(1.50 \mathrm{M}\) \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) ? Explain your reasoning.

A 10.00 mL sample of \(2.05 \mathrm{M} \mathrm{KNO}_{3}\) is diluted to a volume of \(250.0 \mathrm{mL}\). What is the concentration of the diluted solution?

What volume of \(0.750 \mathrm{M} \mathrm{AgNO}_{3}\) must be diluted with water to prepare \(250.0 \mathrm{mL}\) of \(0.425 \mathrm{M} \mathrm{AgNO}_{3} ?\)

Water is evaporated from \(125 \mathrm{mL}\) of \(0.198 \mathrm{M} \mathrm{K}_{2} \mathrm{SO}_{4}\) solution until the volume becomes \(105 \mathrm{mL}\). What is the molarity of \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the remaining solution?

A \(25.0 \mathrm{mL}\) sample of \(\mathrm{HCl}(\mathrm{aq})\) is diluted to a volume of 500.0 mL. If the concentration of the diluted solution is found to be \(0.085 \mathrm{M} \mathrm{HCl}\), what was the concentration of the original solution?

Given a \(0.250 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) stock solution, describe how you would prepare a solution that is \(0.0125 \mathrm{M}\) \(\mathrm{K}_{2} \mathrm{CrO}_{4} .\) That is, what combination(s) of pipet and volumetric flask would you use? Typical sizes of volumetric flasks found in a general chemistry laboratory are \(100.0,250.0,500.0,\) and \(1000.0 \mathrm{mL},\) and typical sizes of volumetric pipets are 1.00,5.00,10.00 \(25.00,\) and \(50.00 \mathrm{mL}\)

Given two liters of \(0.496 \mathrm{M} \mathrm{KCl},\) describe how you would use this solution to prepare \(250.0 \mathrm{mL}\) of \(0.175 \mathrm{M} \mathrm{KCl} .\) Give sufficient details so that another student could follow your instructions.

Consider the reaction below: \(2 \mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{S}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{Ag}_{2} \mathrm{S}(\mathrm{s})+2 \mathrm{NaNO}_{3}(\mathrm{aq}) $$ (a) How many grams of \(\mathrm{Na}_{2} \mathrm{S}(\mathrm{s})\) are required to react completely with \(27.8 \mathrm{mL}\) of \(0.163 \mathrm{M} \mathrm{AgNO}_{3} ?\) (b) How many grams of \(\mathrm{Ag}_{2} \mathrm{S}(\mathrm{s})\) are obtained from the reaction in part (a)?

Excess \(\mathrm{NaHCO}_{3}\) is added to \(525 \mathrm{mL}\) of \(0.220 \mathrm{M}\) \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2} .\) These substances react as follows: \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+2 \mathrm{NaHCO}_{3}(\mathrm{s}) \longrightarrow\) $$ \mathrm{CuCO}_{3}(\mathrm{s})+2 \mathrm{NaNO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g}) $$ (a) How many grams of the \(\mathrm{NaHCO}_{3}(\mathrm{s})\) will be consumed? (b) How many grams of \(\mathrm{CuCO}_{3}(\mathrm{s})\) will be produced?

How many milliliters of \(0.650 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) are needed to precipitate all the silver in \(415 \mathrm{mL}\) of \(0.186 \mathrm{M}\) \(\mathrm{AgNO}_{3}\) as \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s}) ?\) \(2 \mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{K}_{2} \mathrm{CrO}_{4}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})+2 \mathrm{KNO}_{3}(\mathrm{aq}) $$

Consider the reaction below. \(\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \longrightarrow \mathrm{CaCl}_{2}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})\) (a) How many grams of \(\mathrm{Ca}(\mathrm{OH})_{2}\) are required to react completely with \(415 \mathrm{mL}\) of \(0.477 \mathrm{M} \mathrm{HCl} ?\) (b) How many kilograms of \(\mathrm{Ca}(\mathrm{OH})_{2}\) are required to react with 324 L of a HCl solution that is 24.28\% HCl by mass, and has a density of \(1.12 \mathrm{g} / \mathrm{mL} ?\)

Exactly \(1.00 \mathrm{mL}\) of an aqueous solution of \(\mathrm{HNO}_{3}\) is diluted to \(100.0 \mathrm{mL}\). It takes \(29.78 \mathrm{mL}\) of \(0.0142 \mathrm{M}\) \(\mathrm{Ca}(\mathrm{OH})_{2}\) to convert all of the \(\mathrm{HNO}_{3}\) to \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) The other product of the reaction is water. Calculate the molarity of the undiluted HNO \(_{3}\) solution.

A \(5.00 \mathrm{mL}\) sample of an aqueous solution of \(\mathrm{Na}_{2} \mathrm{H}_{3} \mathrm{PO}_{4}\) requires \(49.1 \mathrm{mL}\) of \(0.217 \mathrm{M} \mathrm{NaOH}\) to convert all of the \(\mathrm{Na}_{2} \mathrm{H}_{3} \mathrm{PO}_{4}\) to \(\mathrm{Na}_{3} \mathrm{PO}_{4} .\) The other product of the reaction is water. Calculate the molarity of the \(\mathrm{Na}_{2} \mathrm{H}_{3} \mathrm{PO}_{4}\) solution.

How many grams of sodium must react with \(155 \mathrm{mL}\) \(\mathrm{H}_{2} \mathrm{O}\) to produce a solution that is \(0.175 \mathrm{M} \mathrm{NaOH} ?\) (Assume a final solution volume of \(155 \mathrm{mL}\) ) $$ 2 \mathrm{Na}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow 2 \mathrm{NaOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g}) $$

A method of lowering the concentration of \(\mathrm{HCl}(\mathrm{aq})\) is to allow the solution to react with a small quantity of Mg. How many milligrams of Mg must be added to \(250.0 \mathrm{mL}\) of \(1.023 \mathrm{M} \mathrm{HCl}\) to reduce the solution concentration to exactly \(1.000 \mathrm{M} \mathrm{HCl} ?\) $$ \mathrm{Mg}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \longrightarrow \mathrm{MgCl}_{2}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g}) $$

A 0.3126 g sample of oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) requires 26.21 mL of a particular concentration of \(\mathrm{NaOH}(\mathrm{aq})\) to complete the following reaction. What is the molarity of the \(\mathrm{NaOH}(\mathrm{aq}) ?\) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(\mathrm{s})+2 \mathrm{NaOH}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) $$

A \(25.00 \mathrm{mL}\) sample of \(\mathrm{HCl}(\mathrm{aq})\) was added to a \(0.1000 \mathrm{g}\) sample of \(\mathrm{CaCO}_{3}\). All the \(\mathrm{CaCO}_{3}\) reacted, leaving some excess HCl(aq). \(\mathrm{CaCO}_{3}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{CaCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g}) $$ The excess HCl(aq) required 43.82 mL of 0.01185 M \(\mathrm{Ba}(\mathrm{OH})_{2}\) to complete the following reaction. What was the molarity of the original HCl(aq)? $$2 \mathrm{HCl}(\mathrm{aq})+\mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq}) \longrightarrow \mathrm{BaCl}_{2}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$$

How many moles of \(\mathrm{NO}(\mathrm{g})\) can be produced in the reaction of \(3.00 \mathrm{mol} \mathrm{NH}_{3}(\mathrm{g})\) and \(4.00 \mathrm{mol} \mathrm{O}_{2}(\mathrm{g}) ?\) $$ 4 \mathrm{NH}_{3}(\mathrm{g})+5 \mathrm{O}_{2}(\mathrm{g}) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) $$

The reaction of calcium hydride and water produces calcium hydroxide and hydrogen as products. How many moles of \(\mathrm{H}_{2}(\mathrm{g})\) will be formed in the reaction between \(0.82 \mathrm{mol} \mathrm{CaH}_{2}(\mathrm{s})\) and \(1.54 \mathrm{mol} \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ?\)

A 0.696 mol sample of \(\mathrm{Cu}\) is added to \(136 \mathrm{mL}\) of \(6.0 \mathrm{M}\) HNO \(_{3}\). Assuming the following reaction is the only one that occurs, will the Cu react completely? $$\begin{aligned} 3 \mathrm{Cu}(\mathrm{s})+8 \mathrm{HNO}_{3}(\mathrm{aq}) & \longrightarrow 3 \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) +4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+2 \mathrm{NO}(\mathrm{g}) \end{aligned}$$

A side reaction in the manufacture of rayon from wood pulp is \(3 \mathrm{CS}_{2}+6 \mathrm{NaOH} \longrightarrow 2 \mathrm{Na}_{2} \mathrm{CS}_{3}+\mathrm{Na}_{2} \mathrm{CO}_{3}+3 \mathrm{H}_{2} \mathrm{O}\) How many grams of \(\mathrm{Na}_{2} \mathrm{CS}_{3}\) are produced in the reaction of \(92.5 \mathrm{mL}\) of liquid \(\mathrm{CS}_{2}(d=1.26 \mathrm{g} / \mathrm{mL})\) and 2.78 mol NaOH?

Lithopone is a brilliant white pigment used in waterbased interior paints. It is a mixture of \(\mathrm{BaSO}_{4}\) and \(\mathrm{ZnS}\) produced by the reaction $$\mathrm{BaS}(\mathrm{aq})+\mathrm{ZnSO}_{4}(\mathrm{aq}) \longrightarrow \mathrm{ZnS}(\mathrm{s})+\mathrm{BaSO}_{4}(\mathrm{s})$$ How many grams of lithopone are produced in the reaction of \(315 \mathrm{mL}\) of \(0.275 \mathrm{M} \mathrm{ZnSO}_{4}\) and \(285 \mathrm{mL}\) of 0.315 M BaS?

Ammonia can be generated by heating together the solids \(\mathrm{NH}_{4} \mathrm{Cl}\) and \(\mathrm{Ca}(\mathrm{OH})_{2} . \mathrm{CaCl}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) are also formed. (a) If a mixture containing \(33.0 \mathrm{g}\) each of \(\mathrm{NH}_{4} \mathrm{Cl}\) and \(\mathrm{Ca}(\mathrm{OH})_{2}\) is heated, how many grams of \(\mathrm{NH}_{3}\) will form? (b) Which reactant remains in excess, and in what mass?

Chlorine can be generated by heating together calcium hypochlorite and hydrochloric acid. Calcium chloride and water are also formed. (a) If \(50.0 \mathrm{g}\) \(\mathrm{Ca}(\mathrm{OCl})_{2}\) and \(275 \mathrm{mL}\) of \(6.00 \mathrm{M} \mathrm{HCl}\) are allowed to react, how many grams of chlorine gas will form? (b) Which reactant, \(\mathrm{Ca}(\mathrm{OCl})_{2}\) or \(\mathrm{HCl}\), remains in excess, and in what mass?