Balance the following reaction in acidic solution.Ст20 (ад) + HNO2(ag) >→ Cr** (aq) + NO, (ag)Fill in the coefficients and substances for the balancedoverall equation.Note: Do NOT leave any coeffient fields empty. If thecoefficient is 1, choose "1" as opposed to leaving it blank.3 v vH*♥H20♥HNO, + 5+1 v →3 v NO,Cr,0,2-7.+ 2 v Cr3+ + 4

Balancing the chemical equation involves many steps. There is a difference in the balancing of the…

Answered: Balance the following reaction in…

Science

Chemistry

Balance the following reaction in acidic solution. Cr20 (ag) + HNO2(aq) → Cr**(aq) + NO, (ag) Cr3+

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter8: Electrochemistry And Ionic Solutions

Section: Chapter Questions

Problem 8.10E: For each of the following reactions, determine the overall balanced electrochemical reaction, its...

See similar textbooks

Related questions

Q: This is a question about balancing oxidation reduction reactions for CHM-152

A: In MnO4- we have Mn7+ and in Cr2O72- we have Cr6+ hence the oxidation and reduction half reactions…

Q: sample of iron ore weighing 0.2732 g was dissolved in an excess of a dilute acid solution. All the…

A: Given sample of iron ore weighing 0.2732 g 24.70 mL of 0.0174 M KMnO4 for oxidation to Fe(III) ions…

Q: 1. Balance the following oxidation-reduction reaction using the half reaction method under acidic…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: Balance the following reactions in acidic solution: H2MoO4 (aq) + Cr2+ (aq) = Mo (s) + Cr3+ (aq)

A: Balanced reaction in acidic solution:

Q: Balance the following redox equation by the ion-electron method: 2+ H₂O₂ + Fe²+ →Fe M 3+ + H₂O (in…

A: Redox reactions are those in which both oxidation and reduction reaction occurs simultaneously.

Q: Balance the following oxidation/reduction reaction under acidic conditions. Cr20,2 + NO2 Cr3+ NO3

A: The reaction taking place is given as, => Cr2O72- + NO2- -------> Cr3+ + NO3-

Q: Balance the following electrochemical reaction in acid: MnO 4 (aq) + Zr( s) → Mn –"( aq) + Zr + Zr…

Q: Balance the following reaction in acidic solution: Cr2O72-(aq) + SO2(aq) → Cr3+(aq) + SO3(aq)

A: In the given redox reaction, dichromate ion is the oxidizing agent or substance reduced and sulfur…

Q: Cuag) + NO2(9) in acidic solution Сu(s) + NO3 (aq) (aq)

Q: For the following redox reaction, balance the equation under ACIDIC CONDITIONS. Cu + NO3-…

A: 1) Oxidation Half Reaction : In this half reaction two electrons removed from the Cu and forming…

Q: [2] In acidic solution balance the redox reaction Xe(g) Cr,0, (ag) Xe,Os(s) Cr*(aq) Final balanced…

Q: 4. Balance the following equations (use the oxidation number method): a) MnO4¯ + Fe² b) HNO3 + H,S…

Q: balance the oxidation-reduction reaction Cr+CrO4 2-= Cr(OH)3 that occurs in this basic solution

A: The given equation is, The redox reaction means such as oxidation and reduction. Hence, Oxidation…

Q: d. ClO2→ CIO2 + Cl' in acidic solution

A: We will balance the above reaction by Half reaction method .

Q: Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for…

A: The given reaction: The standard electrode potential for the ions can be given as: The standard…

Q: Write the half-reactions for the process of rusting for Fe. (Inorganic Chemistry)

A: Rusting is a chemical reaction which takes place as a result of the combination of iron with oxygen…

Q: . Calculate AGan and K for each reaction. a. The reaction of Cr"(aq) with Cr0,"(aq) in acid solution…

A: The cell potential for the reaction, in which Cr2+ and Cr2O72- undergoes oxidation and reduction…

Q: 2- 7(aq) 3+ Balance the redox reaction Fe+ Cr,0 →Fe + Cr

Q: Complete and balance the following redox reaction in basic solution Cr20,2-(aq) + Hg(1) → Hg²"(aq) +…

Q: 3. Calculate the equilibrium constant for the following reaction using data from the standard…

A: Equilibrium constant gives the relation between the concentration of different reactants and…

Q: Balance this equation for redox reactions occurring in acidic solution. Cr,07 + CH + > Cr**+ Cl,

A: Redox reactions are the reaction in which oxidation number of any element decreases to reduce the…

Q: [4] Balance the following redox reaction in basic solution. SO;2- (aq)+ Cr207 (aq) → Cr*(aq) +…

A: Redox reaction is combination of both oxidation and reduction

Q: 1.1. Complete and balance the following by ion-electron method. Reactions are taking place in acidic…

A: Steps for writing the balanced redox reaction in acidic medium which is shown below: Write the two…

Q: 16. Reducing agent of reaction in Cr,03 (aq) +1-(aq) acidic Cr3* (aq) + I2(s)

A: Reducing agent substance that gets oxidized and reduces others

Q: Find the standard reduction potentials for the following half-reactions in Appendix J. Cr* (aq) + 2…

A: The reduction half reactions taking place are given as, 1) Cr2+ (aq) + 2 e- ------> Cr (s) 2)…

Q: What is the oxidation state of iron in the following compound Ka[F (CN)&J? +2 +3 +1

A: K3[Fe(CN)6]

Q: write the balanced NET ionic equation for the reaction when Mn(C2H3O2)4 and (NH4)2S are mixed in…

A: In this question, we will write NET ionic equation. You can see details Solution below step by…

Q: Complete and balance the following redox reaction in acidic solution. Cr20,2-(aq) +3 Pb²*(aq) +2…

Q: Cr** + UO?* (acidic) 1. CrņO,²- +U4* → 2. V²* + V(OH)4* → VO²* (basic)

A: The oxidation is the loss of electrons. So in oxidation, the oxidation number of the element…

Q: Balance these equations for redox reactions occurring in ACIDIC MEDIUM. Identify the reducing agent…

A: The substance that oxidises another substance is called oxidizing agent and the substance that…

Q: Give reasons :(i) Zn is not regarded as a transition element.(ii) Cr2+ is a strong reducing agent.

A: (i) Zn belongs too d block but not considered as transition elements because it contains completely…

Q: Balance the redox equation below, it occurs in basic solution. Identify the Reducing Agent and…

Q: Jsing the half-reaction method, balance the following reaction under acidic conditions: TeO,2 N204…

A: Balance the oxygen on both sides by adding H2O to one side. Balance the hydrogen on both sides by…

Q: To obtain Mn2+ using Cl− as a reducing agent, should you use MnO2 or MnO−4?

A: Below attached file showing the details answer. All the best.

Q: Use the standard reduction potentials located in the "Tables' linked above to calculate the standard…

Q: Balance the following reaction in acidic solution Fe2+(aq) + NO3−(aq)  Fe3+(aq) + NO(g)

A: Balance the following reaction in acidic solution--

Q: What happens if a piece of metallic copper is dipped in a solution containing Cr3 + ions?

Q: Balance the following redox reaction in acidic solution. Fe (aq)+1,(s) 2+ Fe (aq)+IO3(aq)

Q: Balance the following equation in acidic solution: Identify the reducing agent: Oxidizing agent:…

Q: Balance the equation below for the reaction under acidic aqueous conditions. Cr20 (aq) (ag) Cr3+…

Q: Balance this equation for the reaction of Zn with Cr2072- in acidic aqueous solution. Zn(s) + Cr,0?…

A: Seven steps are required to balance the given redox reaction in acid solution. First reduction and…

Q: Balance the follow equation for the reaction in an acidic and basic environment. a. Fe2* + Mno, →…

A: Your unbalanced equation : Fe²+ + MnO4 → Fe³+ + Mn²+ 1. Find the oxidation number of every atom.…

Q: Complete and balance the reaction in acidic solution. equation: ZnS + NO3 Zn²+ +S + NO

Q: Balance the following equation which takes place in acidic solution. Cr20-2-+ - Cr3+ + 103

Q: A sample of steel weighing 0.1708 g was dissolved and the manganese present was converted to MnO4–…

Q: Balance each redox reaction occurring in acidic aqueous solution. a. K(s) + Cr"(aq) Cr(s) + K*(aq)

A: Redox reactions are the combination of reduction and oxidation reactions. The type of reaction in…

Q: 2+ Mn BiO3 MnO4 + Bi 3+ ==>

A: According to Law of conservation of mass, total mass remains during the chemical reaction remains…

Q: An external water pipe is built of aluminum (Al). In order to prevent corrosion, the nails that hold…

A: In order to prevent corrosion of aluminium metal pipe, the nails must be made of metal with more…

Q: Balance the following oxidation-reduction equation. The reaction occurs in basic solution. Cr20,2-…

A: Solution of your question is given below :

Q: Calculate the equilibrium constant for the following reactions at 25°C from reduction potential…

A: The reaction taking place is given as, => Cu2+ (aq) + Cu (s) -----> 2 Cu+ (aq) Given :…

Question

Balance the following reaction in acidic solution.
Ст20 (ад) + HNO2(ag) >
→ Cr** (aq) + NO, (ag)
Fill in the coefficients and substances for the balanced
overall equation.
Note: Do NOT leave any coeffient fields empty. If the
coefficient is 1, choose "1" as opposed to leaving it blank.
3 v vH*
♥H20♥
HNO, + 5
+1 v →3 v NO,
Cr,0,2-
7.
+ 2 v Cr3+ + 4

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
In some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.
Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V