Stoichiometry of Chemical Reactions

What mass of gallium oxide Ga₂O₃ can be prepared from 29 g of gallium metal? The equation for the reaction is  \(4Ga + 3{O_2} \to 2G{a_2}{O_3}\)

In an acidic solution hydrogen peroxide reacts with Fe⁺² to produce Fe⁺³ and water. Write a balanced equation for this reaction.

Outline the steps needed to determine the limiting reactant when 30.0 g of propane,\({C_3}{H_8}\), is burned with 75.0 g of oxygen. Determine the limiting reactant.

Write a balanced equation for the decomposition of ammonium nitrate to form molecular nitrogen, molecular oxygen and water. (Hint Balance oxygen last, since it is present in more than one molecule on the right side of the equation)

Diatomic chlorine and sodium hydroxide(lye) are commodity chemicals produced in large quantities, along with diatomic hydrogen via the electrolysis of brine according to the following unbalanced equation: 

\[NaCl\left( {aq} \right) + {H_2}O\left( l \right) \to NaOH\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right).\]

Write balanced molecular, complete ionic, and net ionic equations for this process.

Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much heat is required to decompose exactly 1 mole of red HgO(s) to Hg(l) and O₂(g) under standard conditions?

Which solution could be used to precipitate barium ion Ba²⁺, in a water sample, Sodium chloride, sodium hydroxide, or sodium sulfate. What is the formula for the expected precipitate?

Write the net ionic equation representing the neutralization of any strong acid with an ionic hydroxide. 
(Hint: Consider the ions produced when a strong acid is dissolved in water)

This equation describes the production of tin (II) chloride.\(Sn\left( s \right) + 2HCl\left( g \right) \to SnC{l_2}\left( s \right) + {H_2}\left( g \right)\)Is this a redox reaction? If so, provide a more specific name to the reaction if appropriate, and identify the oxidant and reductant.

Assign oxidation state to elements whose atoms are underlined in each of the following compounds or ions:

1. KNO₃
2. AlH₃
3. NH₄⁺
4. H₂PO₄^-

How many moles of Ca(OH)₂ are required to react with 1.36 mol of H₃PO₄ to produce Ca₃(PO₄)₂ according to the equation  \(3Ca{\left( {OH} \right)_2} + 2{H_3}P{O_4} \to C{a_3}{\left( {P{O_4}} \right)_2} + 6{H_2}O\)?

How many NH₃ molecules are produced by the reaction of 4 mol of Ca(OH)₂ according to the following reaction

\({\left( {N{H_4}} \right)_2}S{O_4} + Ca{\left( {OH} \right)_2} \to 2N{H_3} + CaS{O_4} + 2{H_2}O\)

What mass of CO is required to react with 25.13g of Fe₂O₃ according to the equation

\(F{e_2}{O_3} + CO \to 2Fe + 3C{O_2}\)

Which is the limiting reactant when 5.00 g of H₂ and 10 g of O₂ react to form water?

What is the percent yield of a reaction that produces 12.5g of the gas freon CF₂Cl₂ from 32.9 g of CCl₄ and excess HF.

\(CC{l_4} + 2HF \to C{F_2}\)

A 20.00ml sample of aqueous oxalic acid H₂C₂O₄ was titrated with a 0.09113M solution of potassium permanganate KMnO₄,

\(2MnO_4^ - \left( {aq} \right) + 5{H_2}{C_2}{O_4}\left( {aq} \right) + 6{H^ + } \to 10C{O_2}\left( g \right) + 2M{n^{2 + }}\left( {aq} \right) + 8{H_2}O\left( l \right)\)

A volume of 23.24 ml was required to reach the endpoint. What is the oxalic acid molarity?

What is the percent of chloride ion in a sample if 1.324g of sample produces 1.0881g of AgCl when treated with excess Ag⁺\(A{g^ + } + C{l^ - } \to AgCl\)

A 0.00215g sample of polystyrene, a polymer composed of carbon and hydrogen, produced 0.00726g of CO₂ 0.00148g of H₂O in combustion analysis. What is the empirical formula for polystyrene?

What does it mean to say an equation is balanced? Why is it important for an equation to be balanced?

Consider molecular, complete ionic and net ionic equations.

(a) What is the difference between these types of equations?

(b) In what circumstances would the complete ionic and net ionic equations for a reaction be identical?

Balance the following equations:

\(\begin{array}{l}\;(a)\;PC{l_5}\left( s \right) + {H_2}O\left( l \right) \to POC{l_3}\left( l \right) + HCl\left( {aq} \right)\\\left( b \right)\,Cu\left( s \right) + HN{O_3}\left( {aq} \right) \to Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + {H_2}O\left( l \right) + NO\left( g \right)\\\left( c \right){H_2}\left( g \right) + {I_2}\left( g \right) \to HI\left( s \right)\\\left( d \right)\,Fe\left( s \right) + {O_2}\left( g \right) \to F{e_2}{O_3}\left( s \right)\\\left( e \right)\,Na\left( s \right) + {H_2}O\left( l \right) \to NaOH\left( {aq} \right) + {H_2}\left( g \right)\\\left( f \right)\,{\left( {N{H_4}} \right)_2}C{r_2}{O_7}\left( s \right) \to C{r_2}{O_3}\left( s \right) + {N_2}\left( g \right) + {H_2}O\left( g \right)\\\left( g \right){P_4}\left( s \right) + C{l_2}\left( g \right) \to PC{l_3}\left( l \right)\\\left( h \right)PtC{l_4}\left( s \right) \to Pt\left( s \right) + C{l_2}\left( g \right)\end{array}\)

Balance the following equations:

\(\begin{array}{l}\left( a \right)\,Ag\left( s \right) + {H_2}S\left( g \right) + {O_2}\left( g \right) \to A{g_2}S\left( s \right) + {H_2}O\left( l \right)\\\left( b \right)\,{P_4}\left( s \right) + {O_2}\left( g \right) \to {P_4}{O_{10}}\left( s \right)\\\left( c \right)\,Pb\left( s \right) + {H_2}O\left( l \right) + {O_2}\left( g \right) \to Pb{\left( {OH} \right)_2}\left( s \right)\\\left( d \right)\,Fe\left( s \right) + {H_2}O\left( l \right) \to F{e_3}{O_4}\left( s \right) + {H_2}\left( g \right)\\\left( e \right)\,S{c_2}{O_3}\left( s \right) + S{O_3}\left( g \right) \to S{c_2}{\left( {S{O_4}} \right)_3}\left( s \right)\\\left( f \right)\,C{a_3}{\left( {P{O_4}} \right)_2}\left( {aq} \right) + {H_3}P{O_4}\left( {aq} \right) \to Ca{\left( {{H_2}P{O_4}} \right)_2}\left( {aq} \right)\\\left( g \right)\,Al\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to A{l_2}{\left( {S{O_4}} \right)_3}\left( s \right) + {H_2}\left( g \right)\\\left( h \right)\,TiC{l_4}\left( s \right) + {H_2}O\left( g \right) \to Ti{O_2}\left( s \right) + HCl\left( g \right)\end{array}\)

Write a balanced equation describing each of the following chemical reactions.

(a) Solid potassium chlorate, KClO₃ decomposes to form solid potassium chloride and diatomic oxygen gas

(b) Solid aluminium metal reacts with solid diatomic iodine to form solid Al₂I₆

(c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.

(d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.

Colourful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of metals magnesium, aluminium, and iron with oxygen.

(a)Write the formulae of barium nitrate and potassium chlorate.

(b)The decomposition of solid potassium chlorate leads to the formation of solid potassium chloride and diatomic oxygen gas. Write an equation for the reaction.

(c) The decomposition of solid barium nitrate leads to the formation of solid barium oxide, diatomic nitrogen gas and diatomic oxygen gas. Write an equation for the reaction.

(d)Write separate equations for the reactions of the solid metals magnesium, aluminium and iron and oxygen gas to yield the corresponding metal oxides.(Assume the iron oxide contains \(F{e^{3 + }}\)ions.)

Fill in the blank with a single chemical formula for a covalent compound that will balance the equation:

Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide).

(a) Write an equation of the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water.

(b)The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solution of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.

A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process.

(a)The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide.

(b)The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water.

(c)Solid calcium hydroxide is the added to the sea water, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride 

(d)The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.

(e)Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.

The balanced molecular equations, write the complete ionic and net ionic equations for the following

(a)\({K_2}{C_2}{O_4}\left( {aq} \right) + Ba{\left( {OH} \right)_2}\left( {aq} \right) \to 2KOH\left( {aq} \right) + B{a_2}{C_2}{O_4}\)

(b)\(Pb{\left( {N{O_3}} \right)_2}\left( {aq} \right) + {H_2}S{O_4}\left( {aq} \right) \to PbS{O_4} + 2HN{O_3}\)

(c)\(CaC{O_3}\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to CaS{O_4} + C{O_2} + {H_2}O\)

Use the following equations to answer the next four questions:

i.\({H_2}O\left( s \right) \to {H_2}O\left( l \right)\)

ii.\(N{a^ + }\left( {aq} \right) + C{l^ - }\left( {aq} \right) + A{g^ + }\left( {aq} \right) + NO_3^ - \left( {aq} \right) \to AgCl\left( s \right) + N{a^ + }\left( {aq} \right) + NO_3^ - \left( {aq} \right)\)

iii.\(C{H_3}OH\left( g \right) + {O_2}\left( g \right) \to C{O_2}\left( g \right) + {H_2}O\left( g \right)\)

iv. \(2{H_2}O\left( l \right) \to 2{H_2}\left( g \right) + {O_2}\left( g \right)\)

v. \({H^ + }\left( {aq} \right) + O{H^ - }\left( {aq} \right) \to {H_2}O\left( l \right)\)

(a) Which equation describes a physical change?

(b)Which equation identifies the reactants and products of a combustion reaction?

(c)Which equation is not balanced?

(d)Which is a net ionic equation?

Indicate what type or types of reaction each of the following represents:

(a) \(\)\(Ca\left( s \right) + B{r_2}\left( l \right) \to CaB{r_2}\left( s \right)\)

(b) \(Ca{\left( {OH} \right)_2} + 2HBr\left( {aq} \right) \to CaB{r_2}\left( {aq} \right) + 2{H_2}O\left( l \right)\)

(c) \({C_6}{H_{12}}\left( l \right) + 9{O_2}\left( g \right) \to 6C{O_2}\left( g \right) + 6{H_2}O\left( l \right)\)\(\)

Indicate what type or types of reaction each of the following represents:

(a) \({H_2}O\left( g \right) + C\left( s \right) \to CO\left( g \right) + {H_2}\left( g \right)\)

(b) \(2KCl{O_3}\left( s \right) \to 2KCl\left( s \right) + 3{O_2}\left( g \right)\)

(c) \(Al{\left( {OH} \right)_3}\left( {aq} \right) + 3HCl\left( {aq} \right) \to AlC{l_3}\left( {aq} \right) + 3{H_2}O\left( l \right)\)

(d) \(Pb\left( {N{O_3}} \right)\left( {aq} \right) + {H_2}S{O_4}\left( {aq} \right) \to PbS{O_4}\left( s \right) + 2HN{O_3}\left( {aq} \right)\)

Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

Determine the oxidation state of the elements in the following compounds:

(a)\(NaI\)

(b)\(GdC{l_3}\)

(c)\(LiN{O_3}\)

(d)\({H_2}Se\)

(e)\(M{g_2}Si\)

(f)\(Rb{O_2}\), rubidium superoxide

(g)\(HF\)

Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(a)\({H_3}P{O_4}\)

(b)\(Al{\left( {OH} \right)_3}\)

(c)\(Se{O_2}\)

(d)\(KN{O_2}\)

(e)\(I{n_2}{S_3}\)

(f)\({P_4}{O_6}\).

Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(a) \({H_2}S{O_4}\)

(b) \(Ca{\left( {OH} \right)_2}\)

(c) \(BrOH\)

(d) \(ClN{O_2}\)

(e) \(TiC{l_4}\)

(f) \(NaH\)

Classify the following as acid-base reaction or oxidation-reduction reactions.

(a)\(N{a_2}S\left( {aq} \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}S\left( g \right)\)

(b)\(2Na\left( s \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}\left( g \right)\)

(c)\(Mg\left( s \right) + C{l_2}\left( g \right) \to MgC{l_2}\left( s \right)\)

(d)\(MgO\left( s \right) + 2HCl\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + {H_2}O\left( l \right)\)

(e)\({K_3}P\left( s \right) + 2{O_2}\left( g \right) \to {K_3}P{O_4}\left( s \right)\)

(f)\(3KOH\left( {aq} \right) + {H_3}P{O_4}\left( {aq} \right) \to {K_3}P{O_4}\left( {aq} \right) + 3{H_2}O\left( l \right)\)

Identify the atoms that are oxidized and reduced, the change in the oxidation state for each, and the oxidizing and reducing agents in each of the following equations:

(a)\(Mg\left( s \right) + NiC{l_2}\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + Ni\left( s \right)\)

(b)\(PC{l_3}\left( l \right) + C{l_2}\left( g \right) \to PC{l_5}\left( s \right)\)

(c)\({C_2}{H_4}\left( g \right) + 3{O_2}\left( g \right) \to 2C{O_2}\left( g \right) + 2{H_2}O\left( g \right)\)

(d)\(Zn\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to ZnS{O_4}\left( {aq} \right) + {H_2}\left( g \right)\)

(e) \(2{K_2}{S_2}{O_3}\left( s \right) + {I_2}\left( s \right) \to {K_2}{S_4}{O_6}\left( s \right) + 2KI\left( s \right)\)

(f) \(3Cu\left( s \right) + 8HN{O_3}\left( {aq} \right) \to 3Cu{\left( {N{O_3}} \right)_2}\left( {aq} \right) + 2NO\left( g \right) + 4{H_2}O\left( l \right)\)

Complete and balance the following acid-base equations:

(a)HCl gas reacts with solidCa(OH)₂

(b) A solution of Sr(OH)₂  is added to a solution ofHNO_3.

Complete and balance the following acid-base equations:

(a) A solution ofHClO₄ is added to a solution of LiOH

(b) Aqueous H₂SO₄  reacts with NaOH

(c)Ba(OH)₂ reacts with HF gas.

Complete and balance each of the following oxidation-reduction reactions,such that it results in the highest possible oxidation state for the oxidized atoms.

(a) \(Al\left( s \right) + {F_2}\left( g \right) \to \)

(b) \(Al\left( s \right) + CuB{r_2}\left( {aq} \right) \to \)  (single displacement)

(c) \({P_4}\left( s \right) + {O_2}\left( g \right) \to \)

(d) \(Ca\left( s \right) + {H_2}O\left( l \right) \to \) (products are a strong base and a diatomic gas)

Complete and balance each of the following oxidation-reduction reactions, such that it results in the highest possible oxidation states for the oxidizing atoms:

(a)\(K\left( s \right) + {H_2}O\left( l \right) \to \)

(b)\(Ba\left( s \right) + HBr\left( {aq} \right) \to \)

(c) \(Sn\left( s \right) + {I_2}\left( s \right) \to \)

Toluene, C₆H₅CH₃, is oxidized by air under carefully controlled conditions to benzoic acid, C₆H₅CO₂H, which is used to prepare the food preservative sodium benzoate, C₆H₅CO₂Na. What is the percent yield of a reaction that converts 1.000 kg of toluene to 1.21 kg of benzoic acid? \(2{C_6}{H_5}C{H_3} + 3{O_2} \to 2{C_6}{H_5}C{O_2}H + 2{H_2}O\).

In a laboratory experiment, the reaction of 3.0 mol of \({H_2}\) with 2.0 mol of \({I_2}\) produced 1.0 mol of HI. Determine the theoretical yield in grams and the percent yield for this reaction.

Outline the steps needed to solve the following problem, then do the calculations. Ether, \({\left( {{C_2}{H_5}} \right)_2}O\), which was originally used as an anesthetic but has been replaced by safer and more effective medications, is prepared by the reaction of ethanol with sulfuric acid. \(2{C_2}{H_5}OH + {H_2}S{O_4} \to \left( {{C_2}{H_5}} \right)2O + {H_2}S{O_4} \cdot {H_2}O\) What is the percent yield of ether if 1.17 L (d = 0.7134 g/mL) is isolated from the reaction of 1.500 L of C₂H₅OH (d = 0.7894 g/mL)?

Outline the steps needed to determine the limiting reactant when 0.50 mol of Cr and 0.75 mol of H₃PO₄ react according to the following chemical equation. \(2Cr + 2{H_3}P{O_4} \to 2CrP{O_4} + 3{H_2}\). Determine the limiting reactant.

What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? \(Li + {N_2} \to L{i_3}N\).

How many molecules of C₂H₄Cl₂ can be prepared from 15 C₂H₄ molecules and 8 Cl₂ molecules?

How many molecules of the sweetener saccharin can be prepared from 30 C atoms, 25 H atoms, 12 O atoms, 8 S atoms, and 14 N atoms?

The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.

(a) What is the limiting reactant when 0.200 mol of P₄ and 0.200 mol of O₂ react according to

                        P₄ + 5O₂ ⟶ P₄O₁₀

(b) Calculate the percent yield if 10.0 g of P₄O₁₀ is isolated from the reaction.