# Balance the reaction between Ag2O and I^- to form I2 and Ag in basic solution. When you have...

## Question:

Balance the reaction between Ag2O and I{eq}^- {/eq} to form I2 and Ag in basic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown.

_____Ag2O + _____I{eq}^- {/eq} \rightarrow_____I2 + _____Ag

Water appears in the balanced equation as a _____(reactant, product, neither) with a coefficient of . (Enter 0 for neither.)

How many electrons are transferred in this reaction? _____

## Reactivity of Halogens:

Halogens are strong electronegative elements. Hence, they attract electrons quite strongly. Therefore, they are highly oxidizing in nature and acts as an oxidizing agent in most chemical reactions.

## Answer and Explanation: 1

The oxidation half-reaction is shown below:

{eq}I^{-}\rightarrow I_{2} {/eq}

Balancing {eq}I {/eq}, we get: {eq}2I^{-}\rightarrow I_{2} {/eq}

Balancing charge, we get: {eq}2I^{-}\rightarrow I_{2}+2e^- {/eq}

So, the balanced oxidation half-reaction is:

{eq}2I^{-}\rightarrow I_{2}+2e^- {/eq} ............... (1)

The reduction half-reaction is shown below:

{eq}Ag_{2}O\rightarrow Ag {/eq}

Balancing {eq}Ag {/eq}, we get: {eq}Ag_{2}O\rightarrow 2Ag {/eq}

Balancing {eq}O {/eq} and {eq}H {/eq} in the basic medium, we get: {eq}Ag_{2}O+H_2O\rightarrow 2Ag+2OH^- {/eq}

Balancing charge, we get: {eq}Ag_{2}O+H_2O+2e^-\rightarrow 2Ag+2OH^- {/eq}

The balanced reduction half-reaction is:

{eq}Ag_{2}O+H_2O+2e^-\rightarrow 2Ag+2OH^- {/eq} ................. (2)

{eq}Equation-(1)+Equation-(2): {/eq}

{eq}Ag_{2}O+2I^{-}+H_2O\rightarrow 2Ag+I_2+2OH^- {/eq}

So, the balanced equation ("1" is explicitly shown) is shown below:

{eq}1Ag_{2}O+2I^{-}+1H_2O\rightarrow 2Ag+1I_2+2OH^- {/eq}

Water appears in the balanced equation as a **reactant** with a coefficient of **1**.

**Two** electrons are transferred in the given reaction.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 2 / Lesson 12What is a redox reaction (oxidation reduction reaction)? Learn about redox reaction examples, balancing redox reactions, and the redox reaction definition.

#### Related to this Question

- Balance the reaction between I2 and H2PO2^- to form HPO3^{2-} and I^- in basic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown. [{Blank}] I2 + [{Blank}] H2PO2^- \rightarrow
- Balance the reaction between I- and SnO_3^2- to form SnO_2^2- and I_2 in basic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species
- Balance the reaction between NO2^- and S2O3^{2-} to form SO3^{2-} and N2O in basic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown. [{Blank}] NO2^- + [{Blank}] S2O3^{2-} \r
- Balance the reaction between Cr2O7^{2-} and Co to form Cr^{3+} and Co^{2+} in acidic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown. [{Blank}]Cr2O7^{2-} + [{Blank}]Co \rig
- Balance the reaction between MnO2 and Cd to form Mn^{2+} and Cd^{2+} in acidic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown. [{Blank}]MnO2 + [{Blank}]Cd \rightarrow [{Bl
- Balance the reaction between NH_3 and Br_2 to form Br and N_2H_4 in basic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species show
- After balancing the following redox equation (using small whole-number coefficients), add the coefficients of all species in the balanced equation: Bi(OH)_3 + SnO_2^{2-} \rightarrow Bi + SnO_3^{2-} (basic solution)
- Complete and balance the following redox equation using the set of smallest whole?number coefficients. Now sum the coefficients of all species in the balanced equation. (Remember the coefficients that
- Balance the reaction between Cr^2+ and SO_4^2- to form Cr^3+ and SO_2 in acidic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the specie
- Balance the molecular equation for the following redox reaction. What is the sum of the coefficients? Use the smallest whole number coefficients possible.
- Balance the reaction between I- and N2 to form I2 and N2H4 in basic solution. Water appears in the balanced equation as a (reactant, product, neither) with a coefficient of (0 for neither). How many electrons are transferred in this reaction?
- Balance the following equation using the lowest possible integer coefficients and give the coefficient of H_2. V_2O_5 + H_2 to V_2O_3 + H_2O
- (a) Balance the following equation under basic conditions. S n O 2 2 + B r 2 B r + S n O 2 3 (b) Water appears in the balanced equation as a _____ (reactant, product, neither) with a coefficient of _____. (c) Which species is the oxidizing agen
- Balance the following equation for the reaction in an acidic medium by the ion-electron method. (Use the lowest possible coefficients. Omit states-of-matter in your answer.) MnO4- + H2C2O4 --> Mn2+ +
- Balance the following redox equation in acid. In the blank put the correct stoichiometric coefficient (0, 1, 2, etc.) (Note: 0 if the species does not appear on that side of the equation.) Balance the
- Balance the equation for following reaction in acidic solution: As + ClO3- ? H3AsO3 + HClO The sum of the coefficients of all reactants and products in the correctly balanced equation is equal to wh
- Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of H^+. H_2CO(aq) + S(s) to H_2S(g) + CO_2(g) a. 4 b. 6 c. 2 d. 0 e. 1.
- Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water. MnO_4^- (aq) + H_2SO_3(aq) to Mn^2+(aq) + HSO_4^- (aq) a. 1. b. 2. c. 3. d. 6. e. 5.
- Balancing Redox Reactions Balance the following reactions in basic solution: S_2O_4^2- + CrO_4^2- ----> SO_3^2- + Cr(OH)_4^-
- The following reaction occurs in a basic solution. Balance it by adding only OH^- or H_2O. (Enter the answer as the sum of the coefficients) MnO_4^- (aq) + NO_2^- (aq) to MnO_2 (s) + NO_3^- (aq)
- The following reaction occurs in basic solution. Balance it by adding only OH^- or H_2O. (enter your answer as the sum of the coefficients) MnO_4^- (aq) + NO_2 (aq) --> MnO_2(s) + NO_3^-(aq)
- Balance the depicted redox equation which occurs in the basic solution. CrO42-(aq)+SO32-(aq)---Cr(OH)3(s)+SO42-(aq)
- Balance the following in acidic solution. (Omit states-of-matter from your answer. Use the lowest possible whole number coefficients.) (a) Hg + SnO2 ---> Hg2^2+ + Sn^2+ (b) Fe + Cr2O7^2- ---> Fe^3+
- Balance the equation under acidic condition. When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown? CIO_4^- + Fe ? CIO_3^- + Fe^2+
- Write the half-reactions and the balanced equation for the galvanic cell: Hg(l) | Hg_2^(2+)(aq) || MnO^(4 )(aq), Mn^(2+)(aq), H^+(aq) |. What is the smallest possible integer coefficient of H_2O(l) in the combined balanced equation?
- Compose the balanced reaction equation for the following reaction occurring in acidic aqueous medium. Reduce all coefficients to the lowest possible integers. As2S3(s) + NO3?(aq) ? H3AsO4(aq) + NO(g)
- Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH)3 + SnO2^2? Bi + SnO3^2? (in basic solution) A)32 B) 25 C) 16 D) 13 E) None of these.
- Balance the following equation in basic solution using the lowest possible integers and give the coefficient of hydroxide ion.
- Balance the following chemical equation. What is the sum of the coefficients of the balanced equation? The coefficients should be the smallest possible set of whole numbers. C7H16 + O2 to CO2 + H2O (unbalanced) a) 30 b) 54 c) 32 d) 27
- Balance the following redox reaction occurring in basic solution. O2(g)+Ag(s) rightarrow Ag+(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.
- Consider the unbalanced redox reaction: Cr_2O_2^-7(aq)+Cu(s)-->Cr^3+(aq)+Cu^2+(aq) PART A: Balance the equation. Express your answer as a chemical equation. Identify all of the phases in your answ
- Consider the unbalanced redox reaction: MnO_4(aq) + Zn(s) rightarrow Mn^{2+}(aq)+Zn^{2+}(aq) (a) Balance the equation in acidic solution.Express your answer as a chemical equation. Identify all o
- Balance the following reactions. Use the lowest possible coefficients for all reactions. a)\;\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+\mathrm{HCl}(a q) \rightarrow \mathrm{FeCl}_{3}(a q)+\mathrm{H}_
- Balance the following equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) C_{10}H_{22}(l) + O_2(g) to CO_2(g) + H_2O(g)
- Balance the following decomposition reaction by placing an integer between 1 and 9 as the coefficient for each reactant and product in the equation. LiHCO_3 (s) to Li_2CO_3 (s) + CO_2 (g) + H_2O(g)
- Show the balanced half-reactions and a balanced redox equation for the following reaction in acidic solution. Identify all of the phases in your answer. M g ( s ) + V O 3 4 ( a q ) M g 2 + ( a q ) + V 2 + ( a q )
- Show the balanced half-reactions and a balanced redox equation for the following reaction in acidic solution. Identify all of the phases in your answer. S 2 O 2 3 ( a q ) + B r 2 ( l ) S 4 O 2 6 ( a q ) + B r ( a q )
- When the equation for the following reaction in basic solution is balanced, what is the sum of the coefficients? A. 11 B. 31 C. 14 D. 9
- Balance each redox reaction occurring in acidic aqueous solution. Use the half-reaction method.Cr2O72?(aq)+Br?(aq)?Cr3+(aq)+Br2(aq) Express your answer as a chemical equation. Identify all of the phas
- a) Balance the following redox reaction occurring in basic solution: CIO^-(aq) + Cr(OH)_4^-(aq) ? CrO_4^2-(aq) + Cl^-(aq) Express your answer as a chemical reaction. b) Al(s)-MnO_4^-(aq) ? MnO_2(s)
- Complete and balance the following redox equation in basic solution using the set of smallest whole-number coefficients: IO3-(aq) + Sb3+(aq) = I-(aq) + Sb5+(aq)
- Balance the following redox equation: MnO_4^-(aq) + C_2H_3OH(aq) right arrow Mn^{2+} (aq) + CH_3CO_2H (aq) a. Write separate skeletal half reactions. b. Correctly balance each half reaction. c. Use b) to balance the total reaction.
- Balance each of the following redox reactions occurring in acidic solution. PbO_2 (s) + I^- (ag) --> Pb^2+ (aq) + I_2 (s) Express your answer as a chemical equation. Identify all of the phases in yo
- Balance each of the following redox reactions occurring in an acidic solution. Part A I (aq) + NO_2 (aq) --> I_2 (s) + NO(g) Express your answer as a chemical equation. Identity all of the phases in your answer.
- Balance using half-reaction method for aqueous redox equation in acidic solution. I^{1-} + NO_2^{1-} to I_2 + NO
- When the following half reaction is balanced under basic conditions, what are the coefficients of the species? PH_3+OH^- to P+H_2O
- When the following half reaction is balanced under basic conditions, what are the coefficients of the species? NO_2+OH^- to NO_3^- + H_2O
- Balance the following equation for a reaction in acidic solution. Only H+ or H2O may be added. (enter your answer as the sum of the coefficients) HBrO(aq) --> Br^- (aq) + O2(g)
- Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0, 1, 2, etc). (Note: 0 is the species does not appear on that side of the equation.) .......PbO_2
- Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of H^+. Cl_2 (aq) + S_2O_3^2- (aq) to Cl^-(aq) + SO_4^2- (aq) A. 10. B. 8. C. 1. D. 3. E. 2.
- Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of H+. MnO4-(aq) + H2S(g) \rightarrow Mn2+(aq) + HSO4-(aq)
- Balance each of the following redox reactions occurring in basic solution. Part A H_2O (aq) + Cl_O2 (aq) -->ClO_2 (aq) +O_2 (g) Express your answer as a chemical equation. Identify all of the phases
- Balance each redox reaction occurring in basic aqueous solution.
- Balance the following equations in both acidic and basic environments. Show the half-reactions right before they are added together (after balancing all the components) and then show the balanced equation. a. Cr2O72-(aq) + C2H5OH(l) arrow Cr3+(aq) + CO2(g
- Balance the following equation and classify it as a combination, decomposition, single replacement, or double replacement reaction. KIO3 arrow KI + O2
- When the reaction MnO_4^-(aq) + I^-(aq) \to I_2(s) + MnO_2(s) is balanced in basic solution so that the stoichiometric coefficients appear as the the smallest possible integers, the coefficient for OH^- is: A. 3 B. 2 C. 6 D. 9 E. 8
- Balance the following redox equation with the smallest whole number coefficients: Zn(s) + ReO4(aq) arrow Re(s) + Zn2+(aq) (acidic solution)
- Predict the product(s) and write a balanced equation for the following redox reaction: (Remember to enter the states of matter in your equation.)
- When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown? H2BO3- + S2- -->B + S Water appears in the balanced equation as a (reactant, pr
- Balance each of the following redox reactions occurring in acidic aqueous solution. (Express your answer as a chemical equation. Identify all of the phases in your answer.)...
- Balance each redox reaction occurring in acidic aqueous solution. Use the half-reaction method. Express your answer as a chemical equation. Identify all of the phases in your answer. a) IO3^-(aq)+SO2
- Balance the following equation for a half reaction that occurs in acidic solution. Use e^- as the symbol for an electron. Cl_2 \rightarrow HClO
- Write a balanced equation predicting potential products (if any) when chlorine is bubbled in sodium iodide solution.
- Balance the following redox reaction occurring in basic solution. O_2 (g) + Ag(s) --> Ag^+ (aq) Express your answer as a chemical equation. Identify all of the phases in your answer.
- Balance the following equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) RbClO_3 (s) to RbCl (s) + O_2 (g)
- Balance the following redox equations using the half-reaction in acidic aqueous solution: N O 2 ( a q ) + C u ( s ) N O ( g ) + C u 2 + ( a q ) N O 3 ( a q ) + C u ( s ) N O ( g ) + C u 2 + ( a q ) In the reactions above, which element is being oxi
- BrO 3 ? (aq)+Sn 2 +(aq)+ _____ ? Br ? (aq)+Sn 4 +(aq)+ _____ H 2 O(l)and H + (aq) are involved in the reaction. What are the coefficients of the six species in the balanced equation above? Remember
- Balance the following equation on molecular form. Write a balanced ionic and net-ionic equation for each. Include the physical state ((s), (aq), etc) for all species. Na_2CO_3(aq)+Sr(OH)_2(aq)\to SrCO_3(s)+NaOH(aq)
- Balance the following equation for a half reaction that occurs in basic solution. Use e^- as the symbol for an electron. AgO ? Ag_2O
- Balance the following equation for a half reaction that occurs in basic solution. Use e^- as the symbol for an electron.
- Balance the following equation for a half reaction that occurs in basic solution. Use e as the symbol for an electron. {SO_3}^{2-} + 2H_2O \longrightarrow {S_2O_4}^{2-} + 4OH^-
- Balance the following equation for a half reaction that occurs in basic solution. Use e- as the symbol for an electron. SO_3^2- -->S_2O_4^2-
- Balance the following equation for a half reaction that occurs in basic solution. Use e- as the symbol for an electron. S3-2 ---> S2O4-2
- Balance each of the following half-reactions, assuming that they occur in basic solution. A.) O 2 ( g ) ? O H ? ( a q ) B.) H 2 O 2 ( a q ) ? O 2 ( g ) C.) M n O ? 4 ( a q ) ? M n O 4 2 ? ( a q
- Balance the following equation for a half reaction that occurs in acidic solution. Use e- as the symbol for an electron. MnO_4 ----> MnO_2 Balance the following equation for a half reaction that occurs in basic solution. Use e- as the symbol for an elec
- Balance the following redox equation by the ion-electron half-reaction method. Fe(CN)63- + Cr2O3 arrow Fe(CN)64- + CrO42- (basic solution)
- Balance the following redox equation occurring in basic solution. HS^-(aq)+ClO_3^-(aq) \to S(s)+Cl^-(aq)
- Balance the following redox equation occurring in basic solution. Al(s)+OH^-(aq) \to Al(OH)_4^-(aq)+H_2(g)
- Balance the following redox equation occurring in basic solution. Zn(s)+Cu(OH)_2(s) \to [[Zn(OH)_4]^(2-)(aq)+Cu(s)
- Balance the following redox equation occurring in basic solution. CrO_4^(2-)(aq)+SO_3^(2-)(aq) \to Cr(OH)_3(s)+SO_4^(2-)(aq)
- Balance the following equation on molecular form. Write a balanced ionic and net-ionic equation for each. Include the physical state ((s), (aq), etc) for all species. HNO_3(aq)+Sr(OH)_2(aq)\to Sr(NO_3)_2(aq)+H_2O(l)
- Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one." Cr2(SO4)3 + RbOH Cr(OH)3 + Rb2SO4 (a) 10(b) 12(c) 13(d) 14(e)
- Balance equation for the reaction occurring in basic solution. CrO4^{2-} + S^{2-} \to S + CrO^{-}
- 1.When the following equation is balanced properly under acidic conditions, what are the coefficients of the species shown? Ni2+ + Mg Ni + Mg2+ Water appears in the balanced equation as a (reactant,
- Balance each of the following half-reactions, assuming that they occur in basic solution.Express your answer as a chemical equation including phases. 1) CrO42-(aq)<=>Cr(OH)3(s) 2)H2O(l)<=>H2(g) 3)C
- Balance the following equation and classify it as a combination, decomposition, single replacement, or double replacement reaction. PbCl2 + K2CrO4 arrow PbCrO4 + KCl
- Balance the half-reactions assuming that they occur in acidic solution. Express your answer as a balanced half-reaction. Identify all of the phases in your answer. 1) NO3-(aq) arrow NO(g) 2) Zn(s) arr
- 1) Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0, 1, 2, etc.). (Note: 0 if the species does not appear on that side of the equation.) PbO2(s)
- Balance the following equation occurring in basic aqueous solution. Pb(OH)3- + OCl- arrow PbO2 + Cl-
- Using the balanced reaction, enter the formula, charge, and state of the species (exclude H_{2}O) in the solution if neither reactant is present in stoichiometric excess. Pb(NO_{3})_2(aq) + 2NaI(aq) \rightarrow PbI_{2}(s) + 2NaNO_{3}(aq)
- 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 \rightarrow CO2 + H2O
- Balance the reaction below. Determine the sum of the coefficients, this is in an acidic solution. Include coefficients for any unshown species such as water and H+. __ MnO4- + __H2 rightleftharpoons __ Mn2+ + __H+
- Balance the following equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) Eu_2O_3 (s) + H_2S (g) to EuS (s) + H_2O (g) + S (g)
- Balance the following equation. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) Fe (s) + S_8(s) to FeS (s)
- Balance the following equation for a half reaction that occurs in acidic solution. (Use e^- as the symbol for an electron.) Sn \rightarrow HSnO_2^-
- Balance the equation and classify the reaction as a combination C, decomposition D, combustion CO, single SR, and or double replacement DR. Al_4C_3+H_2O to CH_4+Al(OH)_3.
- Balance each of the following redox reactions occurring in acidic aqueous solution. Express your answer as a chemical equation. Identify all of the phases in your answer. Part A : Zn(s) + Sn^{2+}(aq) → Zn^{2+}(aq) + Sn(s) Part B : Mg(s) + Cr^
- Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of iron(II) iodide
- Balance the following redox equation MnO_4^-(aq) + C_2H_3OH(aq) ---> Mn^+2(aq) + CH_3CO_2H(aq) g. Write separate skeletal half reactions h. Correctly balance each half reaction i. Use b) to balanc
- Part A Balance the following equation: K2CrO4+Na2SO3+HCl?KCl+Na2SO4+CrCl3+H2O Generally coefficients of 1 are omitted from balanced chemical equations. When entering your answer, include coefficient