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1.                          0.17/0.17 points |  Previous AnswersOSGenChem1 4.1.P.002.

Consider molecular, net ionic, and complete ionic equations.

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

Molecular   equations are written without regard to the dissociation of any ionic reactants or products, with all formulas represented as neutral substances. Complete ionic           equations

represent all dissolved ionic compounds with the formulas for their dissociated ions, including spectator ions. Net ionic    equations represent only those dissolved ions that are chemically or physically changed by the reaction, omitting any spectator ions.

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

If there are no        spectator ions involved in a reaction, its complete and net ionic equations will be the same.

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2.                          0.17/0.17 points |  Previous AnswersOSGenChem1 4.1.P.004.

Balance the following equations. (Use the lowest possible whole number coefficients. Include states-ofmatter under the given conditions in your answer.)

(a)    Cr₂O₃(s) + SO₃(l) → Cr₂(SO₄)₃(s)

(b)    Bi(s) + H₂O(l) → Bi₃O₄(s) + H₂(g)

(c)     N₂(g) + O₂(g) → N₂O₄(g)

(d)    Sr₃(PO₄)₂(aq) + H₃PO₄(aq) → Sr(H₂PO₄)₂(aq)

(e)    MnCl₄(s) + H₂O(g) → MnO₂(s) + HCl(g)

(f)     Au(s) + H₂S(g) + O₂(g) → Au₂S(s) + H₂O(l)

(g)    Pb(s) + H₂O(l) + O₂(g) → Pb(OH)₂(s)

(h)    In(s) + H₂SO₄(aq) → In₂(SO₄)₃(s) + H₂(g)

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3.                          OSGenChem1 4.1.P.006.

Write a balanced equation describing each of the following chemical reactions. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)

(a)    Solid potassium bromate, KBrO₃, decomposes to form solid potassium bromide and diatomic oxygen gas.

(b)    Solid gallium metal reacts with solid diatomic iodine to form solid Ga2I6.

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

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

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4.                          0.17/0.17 points |  Previous AnswersOSGenChem1 4.1.P.008.

Write the chemical formula for a covalent compound that will balance the equation. (Omit states-of-matter from your answer.)

C3H6O2 + NaOH → C3H5O₂⁻ + Na⁺ + ?

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5.                          OSGenChem1 4.1.P.010.

A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)

(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)     In the third step, calcium hydroxide (mixed with seawater) reacts with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride.

(d)    In the fourth step, solid magnesium hydroxide is added to an aqueous hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.

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

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6.                          OSGenChem1 4.1.WA.001.

One mole of propane (C3H8) gas reacts with five moles of oxygen (O2) gas to produce three moles of carbon dioxide gas (CO2) and four moles of water gas (H2O). Using this description of the reaction, write the corresponding chemical equation, showing the appropriate coefficients for each reactant and product. (Include states-of-matter under the given conditions in your answer.) 

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7. –/0.17 pointsOSGenChem1 4.1.WA.003.

Determine the number of molecules of oxygen (O2) required to complete the following chemical equation.

N2 + O2 → 2 NO2

The number of molecules of oxygen (O2) required is  . 

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8.                    OSGenChem1 4.1.WA.004.

Methane gas (CH4) reacts with fluorine gas (F2) to produce gaseous carbon tetrafluoride (CF4) and hydrogen fluoride gas (HF). The balanced chemical equation for the reaction is as follows:

CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g).

Calculate the number and types of atoms present in the reactants in this chemical equation. 

C   

F   

H   

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9. –/0.17 pointsOSGenChem1 4.1.WA.007.

The combustion of butane gas (C4H10) involves the reaction of butane with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). The chemical equation is as follows:

2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g). Identify the reactants and products from the following.

(a)  the descriptive statement of the reaction

                                               The ---Select---       are butane and oxygen.

                                               The ---Select---      are carbon dioxide and water.

(b)  the chemical equation

                                               The ---Select---       are C4H10 and O2.

                                               The ---Select---       are CO2 and H2O.

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10.–                 OSGenChem1 4.1.WA.011.

Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. The reaction may be represented by the following unbalanced chemical equation:

2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + x H2(g).

What minimum value of the coefficient x would balance the equation? 

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11.–/0.17 pointsOSGenChem1 4.1.WA.013.

Balance the following reaction, using the smallest integer coefficients that correctly represent the stoichiometric ratios in the balanced reaction. (Omit states-of-matter from your answer.)

C4H8 + O2 → CO2 + H2O

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12.–                 OSGenChem1 4.1.WA.014.

Beryllium carbide (Be2C) reacts with water (H2O) to produce methane (CH4) and beryllium hydroxide (Be(OH)2). The unbalanced chemical equation for this reaction can be written as the following.

Be2C + H2O → CH4 + Be(OH)2 Balance the chemical equation.

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13.–/0.17 pointsOSGenChem1 4.1.WA.017.

When aqueous solutions of lead(II) nitrate (Pb(NO3)2) and potassium phosphate (K3PO4) are mixed, the products are solid lead(II) phosphate and aqueous potassium nitrate. Write the balanced chemical equation for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.)

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14.–                 OSGenChem1 4.1.WA.022.

Write the net ionic equation for the reaction of aqueous solutions of silver perchlorate and sodium iodide. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.)

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15.–/0.17 pointsOSGenChem1 4.1.WA.023.

Identify the spectator ion(s) in the following complete (total) ionic equation. (Separate substances in a list with a comma. Omit states-of-matter from your answer.)

Pb²⁺(aq) + 2 NO₃⁻(aq) + 2 K⁺(aq) + 2 I⁻(aq) → PbI2(s) + 2 K⁺(aq) + 2 NO₃⁻(aq)

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16.–                 OSGenChem1 4.2.P.012.

Use the following equations to answer the next four questions.

i.    H2O(l) → H2O(g)

ii.   Rb⁺(aq) + Cl⁻(aq) + Cu⁺(aq) + NO₃⁻(aq) → CuCl(s) + Rb⁺(aq) + NO₃⁻(aq)

iii.  CH3CH2CH2OH(g) + O2(g) → CO2(g) + H2O(g)

iv.  2 H2O(l) → 2 H2(g) + O2(g)

v.   Ti²⁺(aq) + 2 OH⁻(aq) → Ti(OH)2(s)

(a)     Which equation describes a physical change?

H2O(l) → H2O(g)

Rb⁺(aq) + Cl⁻(aq) + Cu⁺(aq) + NO₃⁻(aq) → CuCl(s) + Rb⁺(aq) + NO₃⁻(aq)   

CH3CH2CH2OH(g) + O2(g) → CO2(g) + H2O(g)

2 H2O(l) → 2 H2(g) + O2(g)

Ti²⁺(aq) + 2 OH⁻(aq) → Ti(OH)2(s)

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

H2O(l) → H2O(g)

Rb⁺(aq) + Cl⁻(aq) + Cu⁺(aq) + NO₃⁻(aq) → CuCl(s) + Rb⁺(aq) + NO₃⁻(aq)   

CH3CH2CH2OH(g) + O2(g) → CO2(g) + H2O(g)

2 H2O(l) → 2 H2(g) + O2(g) Ti²⁺(aq) + 2 OH⁻(aq) → Ti(OH)2(s)

(c)     Which equation is not balanced?

H2O(l) → H2O(g)

Rb⁺(aq) + Cl⁻(aq) + Cu⁺(aq) + NO₃⁻(aq) → CuCl(s) + Rb⁺(aq) + NO₃⁻(aq)   

CH3CH2CH2OH(g) + O2(g) → CO2(g) + H2O(g)

2 H2O(l) → 2 H2(g) + O2(g) Ti²⁺(aq) + 2 OH⁻(aq) → Ti(OH)2(s)

(d)     Which is a net ionic equation?

H2O(l) → H2O(g)

Rb⁺(aq) + Cl⁻(aq) + Cu⁺(aq) + NO₃⁻(aq) → CuCl(s) + Rb⁺(aq) + NO₃⁻(aq)   

CH3CH2CH2OH(g) + O2(g) → CO2(g) + H2O(g)

2 H2O(l) → 2 H2(g) + O2(g)

Ti²⁺(aq) + 2 OH⁻(aq) → Ti(OH)2(s)

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17.–                 OSGenChem1 4.2.P.016.

Determine the oxidation states of the elements in the following compounds. (Enter your answer using the format +1 and -2.)

(a) H2S

H S

Ca

C

(c)     NaBH4

Na

B

H

(d)    BaO2 (barium peroxide)

Ba O

Na H

Fe

F

H

Cl

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18.–/0.17 pointsOSGenChem1 4.2.P.020a.

Identify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in the following equation.

Mg(s) + NiCl2(aq) → MgCl2(aq) + Ni(s)

Oxidizing agent

Mg

NiCl2   

Reducing agent

Mg

NiCl2   

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19.–                OSGenChem1 4.2.P.020b.

Identify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in the following equation.

PCl3(l) + Cl2(g) → PCl5(s)

Oxidizing agent PCl3

Cl2   

Reducing agent PCl3

Cl2   

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20.–                 OSGenChem1 4.2.P.022.

Complete and balance the following acid-base equations. (Assume that these reactions go to completion. Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)

(a)    Solid Fe2O3 is treated with a solution of H2SO4

(b)    Solid Zn(OH)2 is treated with a solution of HNO3.

(c)     A solution of H3AsO4 reacts with solid NaOH.

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21.–/0.17 pointsOSGenChem1 4.2.P.030.

In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg₃N₂, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Magnesium reacts with oxygen

Magnesium reacts with nitrogen

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22.–                 OSGenChem1 4.2.P.032.

Calcium propionate is sometimes added to bread to retard spoilage. This compound can be prepared by the reaction of calcium carbonate, CaCO3, with propionic acid, HC^[1]H5CO2, which has properties similar to those of acetic acid. Write the balanced equation for the formation of calcium propionate. (Include states-ofmatter under the given conditions in your answer. Use the lowest possible whole number coefficients.)

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23.–/0.17 pointsOSGenChem1 4.2.P.034.

Solid copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid sulfuric acid as the only product. Write the two equations which represent these reactions. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) 1^st reaction step

24.–                 OSGenChem1 4.2.P.038.

Complete and balance each of the following half-reactions. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients. For the purpose of this exercise, protons need to be written as H⁺ instead of H₃O⁺, unless prompted otherwise.)

(a)     Cr²⁺(aq) → Cr³⁺(aq)

(b)     Hg(l) + Br⁻(aq) → HgBr₄2⁻(aq)

(c)     ZnS(s) → Zn(s) + S2⁻(aq)

(d)     H₂(g) → H₂O(l) (in basic solution)

(e)     H₂(g) → H₃O⁺(aq) (in acidic solution)

(f)      NO₃⁻(aq) → HNO₂(aq) (in acidic solution)

(g)     MnO₂(s) → MnO₄⁻(aq) (in basic solution)

(h)    Cl⁻(aq) → ClO₃⁻(aq) (in acidic solution)

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25.–                 OSGenChem1 4.2.P.040.

Balance each of the following equations according to the half-reaction method. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients. For the purpose of this exercise, protons need to be written as H⁺ instead of H₃O⁺.)

(a)     Zn(s) + NO₃⁻(aq) → Zn²⁺(aq) + N₂(g) (in acidic solution)

(b)     Zn(s) + NO₃⁻(aq) → Zn²⁺(aq) + NH₃(aq) (in basic solution)

(c)     CuS(s) + NO₃⁻(aq) → Cu²⁺(aq) + S(s) + NO(g) (in acidic solution)

(d)     NH₃(aq) + O₂(g) → NO₂(g) (in gas phase)

(e)     Cl₂(g) + OH⁻(aq) → Cl⁻(aq) + ClO₃⁻(aq) (in basic solution)

(f)      H₂O₂(aq) + MnO₄⁻(aq) → Mn²⁺(aq) + O₂(g) (in acidic solution)

(g)     NO₂(g) → NO₃⁻(aq) + NO₂⁻(aq) (in basic solution)

(h)    Fe³⁺(aq) + I⁻(aq) → Fe²⁺(aq) + I₂(aq) (in solution)

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26.–                 OSGenChem1 4.2.WA.005.

Summarize the solubility guidelines for common ions. (This question is graded according to a set of solubility rules provided by WebAssign. The solubility rules provided with your textbook might be slightly different. Select all that apply.) 

All nitrates and acetates are soluble, except for the following ions. 

Ag⁺

Hg₂2+

Pb2+

Ca2+

Sr2+

Ba2+

NH4+

alkali metals

There are no known exceptions.

All chlorides, bromides, and iodides are soluble, except for the following ions. 

Ag⁺

Hg₂2+

Pb2+

Ca2+

Sr2+

Ba2+

NH4+

alkali metals

There are no known exceptions.

All sulfates are soluble, except for the following ions. 

 Ag⁺

Hg₂2+

Pb2+

Ca2+

Sr2+

Ba2+

NH4+

alkali metals

There are no known exceptions.

All sulfides are insoluble, except for the following ions. 

Ag⁺

Hg₂2+

Pb2+

Ca2+

Sr2+

Ba2+

NH4+

alkali metals

There are no known exceptions.

All carbonates are insoluble, except for the following ions. 

Ag⁺

Hg₂2+

Pb2+

Ca2+

Sr2+

Ba2+

NH4+

alkali metals

There are no known exceptions.

All phosphates are insoluble, except for the following ions. 

Ag⁺

Hg₂2+

Pb2+

Ca2+

Sr2+

Ba2+

NH4+

alkali metals

There are no known exceptions.

All hydroxides are insoluble, except for the following ions. 

Ag⁺

Pb2+

Ca2+

Sr2+

Ba2+

alkali metals

There are no known exceptions.

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27.–/0.17 pointsOSGenChem1 4.2.WA.011.

Determine the oxidation number of V in the V5O₁₄³⁻ ion given that the oxidation number of oxygen is

−2. (Enter your answer using the format +1 and -2.)

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28.–/0.41 pointsOSGenChem1 4.2.WA.014.

Write the oxidation numbers of the following. (Enter your answer using the format +1 and -2.)

(a)       F in F2

(b)       N in NH₄⁺

(c)       V in V2O₇⁴⁻

(d)       Co in Co(NO3)2

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