Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Jules Bruno

Types of chemical reactions

When we start to cover other topics such as stoichiometry, molarity, solution chemistry as well as mass conversions, it’s going to become important that you are able to recognize the different types of chemical reactions that exist. Here we’ve compiled a list of the most popular and common types of chemical reactions that you should know at this point. 

  • Metathesis 

  • Acid-Base

  • Hydrogen Displacement

  • Combustion

  • Disproportionation

  • Combination

  • Decomposition

Metathesis chemical reactions

We’re starting out with Metathesis. Metathesis is the formal name of a double displacement or replacement reaction. In these types of reactions, we’re gonna say that our ions basically switch partners. Here, our barium ion now connects with the sulfate ion and then our sodium ion here, connects with our nitrate ion. 

Remember, to get this, we would have to break them up into their ions and then opposites attract. So barium and nitrate, break up into these ions and then sodium and sulfate ion break up into these ions. Opposites would attract. This positive would be attracted to this negative which is how we got barium sulfate. And this negative and this positive were attracted together to give us sodium nitrate as a product.

Acid base chemical reactions

Moving on from that, we have acid-base reactions. When following the traditional definition, this type of reaction produces an ionic salt and water. An ionic salt just means an ionic compound. Here we have nitric acid, which is a common type of strong acid. Then we have lithium hydroxide which is a common type of strong base. If you’re not familiar with the names, make sure you take a look at my sections that go over naming of ionic compounds as well as acids. These combine together to give me lithium nitrate which is our ionic salt and water itself. Dead giveaway here is our acid tends to just be a covalent compound beginning with hydrogen. Our base, the most common types are a metal connected to OH to produce an ionic compound in water.

Hydrogen displacement chemical reactions

Next we have hydrogen displacement. Basically, a metal reacts with HX. X here could be Cl, Br or I. Remember, these are Group7A elements and they produce a metal halide and hydrogen gas. To be able to do this correctly, you’d have to use an activity series chart. Also, if you’re not familiar with this, make sure to take a look at our videos dealing with activity series. In the process, the magnesium metal would displace the hydrogen here and connect with a chlorine to give us MgCl2. Hydrogen can exist by itself. It exists as H2 in the environment. 

Combustion chemical reactions

Next we have combustion. In combustion, we’re going to say the traditional definition is just oxygen gas reacting with a compound that is made up of just carbon and hydrogen or carbon, hydrogen and oxygen. This is important. You’re gonna produce CO2 and water. Here we have a common type of compound called methanol reacting with oxygen gas to produce CO2 and water which is a dead giveaway for this as combustion. The water itself can be either in a liquid phase or the gaseous phase. We’d have to read the type of question they give to us to make sure which one we have. 

Disproportionation chemical reactions

Next we have disproportionation reactions. Disproportionation is when a reactant produces two products - one which is reduced and one which is oxidized.  

Combination and decomposition chemical reactions

In a combination reaction you have more than one reactant combined to give one type of product and that’s the opposite of decomposition where you have exactly one type of reactant breaking up into multiple types of products.

Summary

It’s important to know these different types of chemical reactions and look for the key terms that we placed in bold or highlighted in some way within these examples.


Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.


Additional Problems
For this question, consider what might happen if a solution of mercury (II) nitrate were to be mixed with a solution of ammonium iodide. You will want to write a balanced equation and a net ionic equation to help you answer the following questions.    Upon mixing these two solutions: a redox reaction occurs an acid-base reaction occurs a decomposition reaction occurs a precipitation reaction occurs no reaction occurs
Put the following reactions in this order: precipitation, acid-base, oxidation-reduction: A. Fe(NO3)3(aq)   +   3 KOH(aq)   →   Fe(OH) 3(s)   +   3 KNO 3(aq)  B. 2 Na(s)   +   Cl 2(g)   →   2 NaCl(s) C. HNO3(aq)   +   LiOH(aq)   →   LiNO 3(aq)   +   H 2O(aq)   1. A, B, C             2. A, C, B             3. B, C, A             4. C, B, A
What is the classification for the reaction given below: HCO3- (aq) → H2CO3 (aq) + CO32– (aq)  a) Metathesis b) Acid-Base Reaction c) Hydrogen Displacement d) Disproportionation e) Composition
When glucose, C6H12O6, is completely oxidized with excess oxygen, what are the products? a) H2O2 and CO2 b) H2O and CO2 c) H2O2 and CO d) H2O and CO
Write a balanced equation for the dissolution of CaCO3.
Write a balanced equation for the dissolution of PbCl2.
Write a balanced equation for the dissolution of AgI.
Neurotransmitters are molecules that are released by nerve cells to other cells in our bodies, and are needed for muscle motion, thinking, feeling, and memory. Dopamine is a common neurotransmitter in the human brain. Predict what kind of reaction dopamine is most likely to undergo in water: redox, acid-base, precipitation, or metathesis?
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties.Write a balanced chemical equation for the complete oxidation of N2 to form N2O5(g).
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties.Write a balanced chemical equation for the complete oxidation of acetylene to form CO2( g) and H2O(g).
What is a combustion reaction?
Burning methane in oxygen can produce three different carbon-containing products: soot (very fine particles of graphite), CO(g), and CO2(g).Why, when the oxygen supply is adequate, is CO2(g) the predominant carbon-containing product of the combustion of methane?
A 6.54 g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.73 L of carbon dioxide gas at 28 oC and 744 torr pressure.Write balanced chemical equation for the reaction that occur between hydrochloric acid and magnesium carbonate.
A 6.54 g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.73 L of carbon dioxide gas at 28 oC and 744 torr pressure.Write balanced chemical equation for the reaction that occur between hydrochloric acid and calcium carbonate.
Write a balanced chemical equation for the reaction of solid lithium with liquid water.
Write a balanced chemical equation for the reaction of solid potassium with liquid water.
Write a balanced equation for the reaction of hydrogen gas with bromine gas.
Write balanced molecular equation for the reaction between hydrobromic acid and potassium hydroxide.
Answer the following questions for the reaction:FeCl3 (aq) with NaOH (aq)a. What type of reaction is? (combination synthesis, decomposition, single displacement, double displacement)b. Write the chemical equation.c. Write the complete ionic equation.d. Write the net ionic equation.
If the empirical formula of sodium oxide is Na 2O, can you tell me how to write a balanced chemical equation for this reaction. You already answered the question but why did you start with 4Na +O2. How do I know to start with 4 Na? And then how do I know it produces 2 Na2O. 
Which of the following chemical equations is an acid-base reaction? a. Ba(OH)2(aq) + K2SO4(aq) → BaSO4(s) + 2 KOH(aq)b. 3 NaOH(aq) + AlCl3(aq) → Al(OH)3(s) + 3 NaCl(aq)c. 2 H+(aq) + Zn(s) → H2(g) + Zn2+(aq)d. 2 HCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 HNO3(aq)e. H3PO4(aq) + NH3(aq) → NH4+(aq) + H2PO4-(aq)  
Complete and balance the following chemical equation. Name the product.Ba + H2O →  
Use the following choices to answer the following questions:a. Metathesis         b. Acid-Base              c. Hydrogen Displacement        d. Combustion                  e. Metal Displacement                            f. Disproportionation              g. Combination or Composition            h. Decomposition 1.   Mg (s)  + 2 HCl (aq) → MgCl 2 (aq)  +  H2 (g) 2.   2 HSO3 –  →  SO32–    +    H2SO3 3.   Ca (s)  +   2 LiNO 3 (aq) → Ca(NO3)2 (aq) +  2 Li (s) 4.   3 H2 (g)  + N2 (g) → 2 NH3 (g) 5.   Ba(NO3)2 (aq)  +  Na2SO4 (aq) → BaSO4 (s)  +  2 NaNO3 (aq) 6.   C3H8 (g)  +  5 O2 (g) →  3 CO2 (g)  +  4 H2O (g) 7.   PBr5 (g) →  PBr3 (g)   +   Br2 (g) 8.  NaOH (aq)  +  HBr (aq) → H 2O (l)  +  NaBr (aq)
Balance the following equations and indicate the type of reaction taking place:i) ____NaBr + ____H3PO4 → ___Na3PO4 + ___HBrii) ___Ca(OH)2 + ___Al2(SO4)3 → ___CaSO4 + __Al(OH)3 
Write the product and then name the product of this reaction.Na + H2 → ______?
Predict the products of the following reaction: Express your answer as a chemical formula. If no reaction occurs, enter no reaction.a. MgCl2 + K ⇌b. Ba + P ⇌c. MgCO3 Δ ⇌ 
What kind of reaction occurs when you mix aqueous solutions of barium sulfide and sulfuric acid?
Complete the following reaction. Express your answer as a chemical equation. Identify all of the phases in your answer.C4H10S(l) + O2(g) →
Which of the following is an acid-base reaction?      A) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)B) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)C) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s)D) C(s) + O2(g) → CO2(g)E) None of the above are acid base reactions.
Which of the following is an example of a decomposition reaction?a. HCI(aq) + NaOH(aq) → NaCI(aq) + H 2O(I)b. 2Pb(NO3)2(s) + heat → 2PbO(S) + 2NO(g) + O 2(g)c. AgNO3(aq) + Li2SO4(aq) → 2LiNO3(aq) + Ag2O4(S)d. 2Li(s) + 2H2O(I) → 2LiOH(aq) + H2(g)e. Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
What are the products of the combustion of octane (C 8H18)A. O2 and C4H9B. H2O and C4H9C. CO2 and H2OD. O2 and CO2
A common demonstration in chemistry courses involves adding  a tiny speck of manganese(IV) oxide to a concentrated hydrogen peroxide (H2O2) solution. Hydrogen peroxide decomposes quite spectacularly under these conditions to produce oxygen gas and steam (water vapor). Manganese(IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction. Write the balanced equation for the decomposition reaction of hydrogen peroxide.
Complete and balance the following equation. Name the ionic product of the reaction.K + H2O →
What are products for this reaction? Ba(OH)2 + H2O →
Which of the following is an example of a decomposition reaction?a. 2Na + Cl2 → 2NaCIb. MgO2 → Mg + O2c. H2 + O → H2Od. MgSO4 + 2NaCI → MgCI2 + Na2SO4
The first metal to be prepared from its ore was copper, perhaps as early as 6000 BC in the Middle East. The ore, which contained copper oxide, was heated with charcoal, which was prepared by the incomplete burning of wood and is mainly elemental carbon C (s). Later, iron and tin were prepared the same way. Write the chemical equations for the preparation of these metals. Assume the ores to be CuO (s), SnO2 (s), and Fe2O3 (s). 
Classify each of these reactions.1) Ba(ClO3)2(s) → BaCl2(s)+3O2(g)2) 2NaCl(aq)+K2S(aq) → Na2S(aq)+2KCl(aq)3) CaO(s)+CO2(g) → CaCO3(s)4) KOH(aq)+AgCl(aq) → KCl(aq)+AgOH(s)5) Ba(OH)2(aq)+2HNO2(aq) → Ba(NO2)2(aq)+2H2O(l)The reactions should be either one of these:  acid-base neutralization, precipitation, redox, none of the above
Classify each of these reactions.
Classify each of these reactions: redox, acid -base neutralization, precipitationPb (NO3)2(aq) + 2KCI(aq) → PbCl2(s) + 2KNO3 (aq)CH4(g) + 2O2(g) → CO2(g) + 2H2O(I)Cu(s) + FeCl2(aq) → Fe(s) + Cu Cl2(aq)2KOH(aq) + H2SO(q) → K2SO4 (aq) + 2H2O(I)
Write a balanced equation for the dissolution of BaSO4.
Write a balanced equation for the dissolution of PbBr2.
Write a balanced equation for the dissolution of Ag2CrO4.
Complete and balance each of the following equations for combustion reactions.C4H6(g) + O2(g) →
Complete and balance each of the following equations for combustion reactions.C(s) + O2(g) →
Complete and balance each of the following equations for combustion reactions.CS2(s) + O2(g) →
Complete and balance each of the following equations for combustion reactions.C3H8O(l) + O2(g) →
Classify the following as acid-base reactions or oxidation-reduction reactions:(a) Na2S(aq) + 2HCl(aq) ⟶ 2NaCl(aq) + H2S(g)
Classify the following as acid-base reactions or oxidation-reduction reactions:(d) MgO(s) + 2HCl(aq) ⟶ MgCl2(aq) + H2O(l)
Classify the following as acid-base reactions or oxidation-reduction reactions:(f) 3KOH(aq) + H3PO4(aq) ⟶ K3PO4(aq) + 3H2O(l)
Indicate what type, or types, of reaction each of the following represents:(a) Ca(s) + Br2(l) ⟶ CaBr2(s)
Uranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear weapons. UF6 is made from the reaction of elemental uranium with ClF3, which also produces Cl2 as a by-product.Is this a metathesis reaction?
Indicate what type, or types, of reaction each of the following represents:(b) Ca(OH)2(aq) + 2HBr(aq) ⟶ CaBr2(aq) + 2H2O(l)
Indicate what type, or types, of reaction each of the following represents:(c) C6H12(l) + 9O2(g) ⟶ 6CO2(g) + 6H2O(g)
Indicate what type, or types, of reaction each of the following represents:(a) H2O(g) + C(s) ⟶ CO(g) + H2(g)
Indicate what type, or types, of reaction each of the following represents:(b) 2KClO3(s) ⟶ 2KCl(s) + 3O2(g)
Write a balanced chemical equation for the reaction that occurs when Mg(s) reacts with Cl2(g).
Indicate what type, or types, of reaction each of the following represents:(c) Al(OH)3(aq) + 3HCl(aq) ⟶ AlCl3(aq) + 3H2O(l)
Indicate what type, or types, of reaction each of the following represents:(d) Pb(NO3)2(aq) + H2SO4(aq) ⟶ PbSO4(s) + 2HNO3(aq)
Indicate whether each reaction is a combination, decomposition, or combustion reaction.
Balance the following equations.
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:Ca(s) + H2O(l) ⟶ Ca(OH)2(aq) + H2(g) 
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:NaNO3(s) ⟶ NaNO2(s) + O2(g) 
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:C2H2(g) + H2(g) ⟶ C2H6(g)
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:(a) HI(g) ⟶ H2(g) + I2(g)
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:Zn(s) + AgNO3(aq) ⟶ Zn(NO3)2(aq) + Ag(s) 
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:NO(g) + O2(g) ⟶ N2O4(l)
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:Sb(s) + Cl2(g) ⟶ SbCl3(s) 
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:AsH3(g) ⟶ As(s) + H2(g) 
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:Zn(s) + Fe(NO3)2(aq) ⟶ Zn(NO3)2(aq) + Fe(s)
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:Mg(s) + H2O(g) ⟶ Mg(OH)2(s) + H2(g) 
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:Cr(NO3)3(aq) + Al(s) ⟶ Al(NO3)3(aq) + Cr(s) 
Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:PF3(g) + F2(g) ⟶ PF5(g)
Predict the product(s) and write a balanced equation for each of the following redox reactions:Sr(s) + Br2(l) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Ag2O(s) ⟶Δ
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.(a) Al(s) + F2(g) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Mn(s) + Cu(NO3)2(aq) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Mg(s) + HCl(aq) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:LiCl(l) + electricity ⟶
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.(b) Al(s) + CuBr2(aq) ⟶      (single displacement)
Predict the product(s) and write a balanced equation for each of the following redox reactions:SnCl2(aq) + Co(s) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:N2(g) + H2(g) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:NaClO3(s) Δ ⟶
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.(c) P4(s) + O2(g) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Ba(s) + H2O(l) ⟶
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.(d) Ca(s) + H2O(l) ⟶      (products are a strong base and a diatomic gas)
Predict the product(s) and write a balanced equation for each of the following redox reactions:S8(s) + O2(g) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:BaCl2(l) electricity ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Cesium + iodine ⟶
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.(a) K(s) + H2O(l) ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Aluminum + aqueous manganese(II) sulfate ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Sulfur dioxide + oxygen ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Butane + oxygen ⟶
A historian discovers a nineteenth-century notebook in which some observations, dated 1822, were recorded on a substance thought to be a new element. Here are some of the data recorded in the notebook: "Ductile, silver-white, metallic looking. Softer than lead. Unaffected by water. Stable in air. Melting point: 153˚C. Density: 7.3 g/cm3. Electrical conductivity: 20% that of copper. Hardness: About 1% as hard as iron. When 4.20 g of the unknown is heated in an excess of oxygen, 5.08 g of a white solid is formed. The solid could be sublimed by heating to over 800˚C." Identify the element reported and write a balanced chemical equation for the reaction with oxygen.
Predict the product(s) and write a balanced equation for each of the following redox reactions:Pentane (C5H12) + oxygen ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Phosphorus trichloride + chlorine ⟶
Predict the product(s) and write a balanced equation for each of the following redox reactions:Aqueous potassium iodide + bromine ⟶
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.(c) Sn(s) + I2(s) ⟶
Fill in the blank with a single chemical formula for a covalent compound that will balance the equation:
Predict the product(s) and write a balanced equation for each of the following redox reactions:Zinc + hydrobromic acid ⟶
3.21Indicate whether each reaction is a combination, decomposition, or combustion reaction.C5H6O(l) + O2(g) → CO2(g) + H2O(g)
3.21Indicate whether each reaction is a combination, decomposition, or combustion reaction.N2(g) + H2(g) → NH3(g)
3.21Indicate whether each reaction is a combination, decomposition, or combustion reaction.K2O(s) + H2O(l) → KOH(aq)
When heated to 700–800 °C, diamonds, which are pure carbon, are oxidized by atmospheric oxygen. (They burn!) Write the balanced equation for this reaction.
The military has experimented with lasers that produce very intense light when fluorine combines explosively with hydrogen. What is the balanced equation for this reaction?
Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. Write an equation for the reaction that involves 2 mol of LiOH per 1 mol of CO2. (Hint: Water is one of the products.)
Classify each of these reactions.
Enter a balanced chemical equation for the reaction between aluminum metal and chlorine gas.
Enter a balanced chemical equation for the reaction between lithium metal and liquid water.
Enter a balanced chemical equation for the reaction between gaseous hydrogen and liquid bromine.
Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required.(a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an appropriate acid)
Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required.(b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction
Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required.(c) gaseous H2S from solid Zn and S via a two-step process (first a redox reaction between the starting materials, then reaction of the product with a strong acid)
Give an example of a precipitation reaction.
Give an example of a acid-base reaction.
Give the best definition of a combustion reaction.
Give an example of a combustion reaction.
Complete and balance each of the following equations for combustion reactions.S(s)+O2(g)
Complete and balance each of the following equations for combustion reactions.C3H6(g) + O2(g)
Complete and balance each of the following equations for combustion reactions.Ca(s) + O2(g)
Complete and balance each of the following equations for combustion reactions.C5H12S(l) + O2(g)(Assume that { m SO}_2 is formed.)
What is the reaction of the decomposition of calcium carbonate?
What's the balanced equation for magnesium and hydrochloric acid?
Enter the equation for the decomposition of water into its elements. Phase symbols are not graded.
Which of the following is an oxidation-reduction reaction?a. Cu(s) + 2AgNO3(aq) → 2Ag(s) + Cu(NO3)2(aq)b. HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq)c. AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)d. Ba(C2H3O2)2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaC2H3O2(aq)e. H2CO3(aq) + Ca(NO3)2(aq) → 2HNO3(aq) + CaCO3(s)
Sodium Bicarbonate reacts with Acetic Acid and causes a chemical reaction. The end products of this reaction are water and what compound?
Is this reaction a double displacement reaction? CH3COOH (aq) + NaHCO3 (s) → CH3COONa (aq) + CO2 (g) + H2O (l)
Classify each of these reactions. A single reaction may fit more than one classification.
How to complete this reaction? HNO3 + H2O ?
What are the predicted products for the following single replacement reaction?NaBr(aq) + Cl2 →Choose 1 answer:a. ClBr(aq) and Nab. No reactionc. NaCl(aq) and Br2d. NaCl2(aq) and Br
What are the products of the combustion of octane (C 8H18)?A. O2 and C4H9B. H2O and C4H9C. CO2 and H2OD. O2 and CO2
Identify the precipitation and non-precipitation reactionsa. 4P + 5O2 → 2P2O5b. H2O2 + NaIO → NaI + H 2O + O2c. Ba(NO3)2 + MgSO4 → BaSO4 + Mg(NO3)2d. Hg2(C2H3O2)2 + 2NaBr → Hg 2Br2 + 2NaC2H3O2e. 2KI + Pb(NO3)2 → PbI2 + 2KNO3f. HCI + NaOH → NaCI + H 2Og. HBr + NaOH → NaBr + H 2O
Predict the product(s) and write a balanced equation for each of the following redox reactions:Fe(s) + HClO4(aq) ⟶
Which of the following is an acid-base reaction?A) 2 C2H6(l) + 7 O2(g)  →  4 CO2(g) + 6 H2O(g)B) MgSO4(aq) + Pb(NO3)2(aq)  →  Mg(NO3)2(aq) + PbSO4(s)C) 2 H2(g) + O2(g)  →  2 H2O(g)D) 2 HClO4(aq) + Ca(OH)2(aq)  →  2 H2O(l) + Ca(ClO4)2(aq)E) None of the above is an acid-base reaction.
Use the following equations to answer the next four questions:i. H2O(s) ⟶ H2O(l)ii. Na+(aq) + Cl−(aq) + Ag+(aq) + NO3−(aq) ⟶ AgCl(s) + Na+(aq) + NO3−(aq)iii. CH3OH(g) + O2(g) ⟶ CO2(g) + H2O(g)iv. 2H2O(l) ⟶ 2H2(g) + O2(g)v. H+(aq) + OH−(aq) ⟶ H2O(l)(b) Which equation identifies the reactants and products of a combustion reaction?
Aluminum wire is placed in a copper (II) nitrate solution. Express your answer as a chemical equation. Identify all of the phases in your answer. Enter no reaction if there is no reaction.
Liquid water and carbon dioxide gas are formed by the decomposition of aqueous carbonic acid (H2CO3). Write a balanced chemical equation for this reaction.
Classify the reaction: ammonia gas reacts with hydrochloric acid fumes to form a white solid that settles as a fine dust. NH3 (g) + HCl (g) → NH4Cl (s) (a) Decomposition reaction (b) Precipitation reaction (c) Oxidation-reduction reaction (d) Acid-base reaction (e) Synthesis reaction (f) Double displacement reaction (g) Single displacement reaction (h) Combustion reaction
Classify the following reaction: CaCO3 (s) → CaO (s) + CO2 (g) a. Acid-Base b. Double-Displacement c. Decomposition d. Redox
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms.(b) Ba(s) + HBr(aq) ⟶  
Identify the type of reaction. Complete and balance the reaction if it occurs. a.combinationb. combustionc. decompositiond. single displacemente. double displacementf. no reactionMg(OH)2 + FePO4 → 
Calcium cyclamate Ca(C6H11NHSO3)2 is an artificial sweetener used in many countries around the world but is banned in the United States. It can be purified industrially by converting it to the barium salt through reaction of the acid C6H11NHSO3H with barium carbonate, treatment with sulfuric acid (barium sulfate is very insoluble), and then neutralization with calcium hydroxide. Write the balanced equations for these reactions.
Identify the type of reaction. Complete and balance the reaction if it occurs. (a) combination (b) combustion (c) decomposition (d) single displacement (e) double displacement (f) no reaction F2 + NaBr →
Write a chemical equation for iron metal combining with chlorine gas to give yellow ferrous chloride solid. Express your answer as a chemical equation. Identify all of the phases in your answer.
Identify the type of reaction. Complete and balance the reaction if it occurs. (a) combination (b) combustion (c) decomposition (d) single displacement (e) double displacement (f) no reaction MgI2 + Na2SO4 →
What will be the product(s) of a synthesis reaction in which the reactants are 2H  2 + O2? 
Identify the type of reaction. Complete and balance the reaction if it occurs. (a) combination (b) combustion (c) decomposition (d) single displacement (e) double displacement (f) no reaction C6H12 + O2 →
Identify the type of reaction. Complete and balance the reaction if it occurs. (a) combination (b) combustion (c) decomposition (d) single displacement (e) double displacement (f) no reaction Zn + HNO3 →
Identify the type of reaction. Complete and balance the reaction if it occurs. (a) combination (b) combustion (c) decomposition (d) single displacement (e) double displacement (f) no reaction Mg(OH)2 + FePO4 →
Identify the type of reaction. Complete and balance the reaction if it occurs. (a) combination (b) combustion (c) decomposition (d) single displacement (e) double displacement (f) no reaction LiSO4 + Zn →
H2CO3(aq) ⇌ H2O(l) + CO2(g)In the reaction above, the carbonic acid ______.a. dissolvedb. dissociatedc. decomposed 
Classify the reaction: solid red mercury(ll) oxide forms liquid mercury metal and oxygen gas when heated. HgO (s) → 2Hg (l) + O2 (g) (a) Acid-base reaction (b) Double displacement reaction (c) Single displacement reaction (d) Synthesis reaction (e) Combustion reaction (f) Precipitation reaction (g) Oxidation-reduction reaction (h) Decomposition reaction
Identify the type of reaction. Complete and balance the reaction if it occurs. a.combinationb. combustionc. decompositiond. single displacemente. double displacementf. no reactionZn + HNO3 →  
Baking soda is sodium bicarbonate, NaHCO3, and vinegar is primarily acetic acid, HC2H3O2. At room temperature, the addition of baking soda to vinegar results in a reaction that produces a tremendous amount of gas, as shown in the video. NaHCO3(s) + HC2H3O2(aq) → Complete the following equation for the reaction of NaHCO3(s) with HC2H3O2 (aq). Include phase symbols. NaHCO3(s) + HC2H3O2(aq) → 
From the list below, select all reaction types that apply when magnesium combines with oxygen to form magnesium oxide a. Synthesis (Combination) b. Oxidation-reduction c. Combustion d. Double displacement (double replacement) e. Precipitation f. Decomposition g. Acid-Base (Neutralization) h. Single displacement (single replacement)
What gas is produced when sodium bicarbonate is mixed with hydrochloric acid?a. Hydrogen b. Carbon dioxidec. Oxygen d. Hydrogen carbonate
Write and balance the equation for the complete combustion of acetyene, C 2H2.  You do not need to include any phase symbols or energy changes. 
Write a balanced equation for the reaction of chlorine gas with bromine gas.