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# Write The Balanced Equation For The Reaction Of Aqueous Pb(clo3)2 With Aqueous Nai. Include Phases.

### SCIENCE

• Balance the following redox reaction in acidic conditions Cr2O7 2- (aq) + HNO2 (aq) → Cr3+(aq) + NO3 – (aq)
• ### Chemistry

how do I balance the following skeleton redox equation for a reaction occurring in acidic solution. HNO2 + MnO4- yield to Mn2+ + NO3-

• ### chemistry

Balance the redox reaction of eq. Cu2S + SO4(-2) gives CuO + SO2 (Acidic )

• ### Chemistry

Consider a generic redox reaction then suppose that the coefficients in the redox reaction are doubled. How will the following quantities be affected for a voltaic cell under nonstandard conditions, will they be Doubled, Halved, Squared, or No Change. Note

• ### Chemistry

In a particular redox reaction, MnO2 is oxidized to MnO4– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in acidic solution. Phases are optional. MnO2 + Cu^2+ —> MnO4^- + Cu^+

• ### Chemistry

Balance the following redox reaction. MnO4 (aq) + Fe (s) –> Mn2+ (aq) +Fe2+ (aq)

• ### Chemistry

in a particular redox reaction, MnO2 is oxidized to MnO4– and fe3+ is reduced to fe2+. Complete and balance the equation for this reaction in acidic solution. Phases are optional.

• ### Science

how to balance chemical equations with redox reaction Cr(OH)3 + IO3{-} + OH{-} = CrO4{-2} + I{-}

• ### Chemistry

Classify each of the following as a redox reaction or a non-redox reaction. Zn+CuCl2 -> ZnCl2+Cu HCl+NaOH -> H2O+NaCl 2CO+O2 -> 2CO2 SO3+H2O -> H2SO4

• ### Chemistry 2

In a particular redox reaction, MnO2 is oxidized to MnO4– and Ag is reduced to Ag. Complete and balance the equation for this reaction in acidic solution. Phases are optional.

• ### Chemistry

For the following reaction, the partial pressures are listed in the table: Substance Equlibrium H2S 5.4 I2 1.2 HI 0.43 S 7 If the Kp of the reaction is 0.134, which direction would the reaction need to go to establish equilibrium? H2S(g) + I2(s) 2HI(g) +

• ### Chemistry

Complete and balance the equation for this reaction in basic solution? Redox reaction Cr is oxidized to CrO42– and Fe3 is reduced to Fe2…? For a particular redox reaction Cr is oxidized to CrO42– and Fe3 is reduced to Fe2 . Complete and balance the

• ### Chemistry

Balance the redox reaction Zn+NO3^-=Zn^²+ +NH3

• ### Chem Help!

Which pair of reagents will take part in a redox reaction? A CH3CH2OH + concentrated H2SO4 B CH3CHO + Tollens’ reagent C CH3CO2C2H5 + dilute H2SO4 D CH3COCH3 + Fehling’s solution Ans: B Someone please explain! Thanks! 🙂

• ### chemistry

balance the redox equations: IO3-(aq) -> I2(aq) and I-(aq) -> I2(aq) balance the redox equation: S2O3(-2) -> S4O2(2-) and I3- -> I-

• ### Chemistry – Redox

Balance the following redox reactions by inserting the appropriate coefficients. Al + MnO2 –> Al2O3 + Mn HNO3 + H2S –> NO + S + H20 Initially, I know the first step is to find assign all the oxidation numbers for the products and reactants listed, but am

• ### Chemistry

Balance the following redox reaction in basic solution. H2(g)+Fe3+(aq) —> H2O(l)+Fe2+(aq)

• ### Chemistry

Using the half- reaction method, balance the redox reaction shown below. (I-)+(Br2) —> (IO3-)+(Br-) Step 1. Break the reaction into the two half reactions. Br2 ==> Br^- I^- ==> IO3^- Step 2. I will leave the first one for you to do. The second one is

balance the redox reaction NO2^- + Ag^+ = NO3^- + Ag

• ### Chemistry (redox reaction)

Which reaction is a redox reaction? 1. HCI+H2O=H3O^+ +CI^- 2. H2SO4+2KOH=K2SO4+2H2O 3. CH4+2O2=CO2+2H2O 4. Fe^2+ +2OH^- =Fe(OH)2 I chose number 3, is this correct?

• ### chemistry

Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous NaI. Include phases. What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)2 is mixed with 0.350 L of 0.290 M NaI? Assume the reaction goes to completion.

• ### CHEMISTRY

Hello, I am trying to balance this redox reaction WITHOUT using the half-reaction method. Here is the unbalanced equation: MnO4 -(aq) + Zn(s)–> Mn 2+(aq) + Zn 2+(aq) It looks as if both elements are being oxidized. The answer is supposed to be: 2MnO4

• ### Chemistry

Is the decomposition of lead(ii)nitrate a redox reaction? Equation with O.S. underneath 2Pb(NO3)2 => 2PbO + 4NO2 + O2 +2 -1 +2-2 +4-2 0 I got all the o.s. but I am still confused as to whether or not this makes it a redox reaction. Do the individual

• ### Chemistry

What is the balance of the following redox reaction Fe2+(aq)+Cr2O72-(aq) Cr3+(aq)+Fe3+(aq)

• ### Chem

How would one balance the following redox reaction using the half reaction method? Fe(OH)2 + O2 + H2O —> Fe(OH)3 This is in my chemistry teacher’s homework, and it comes up with an answer, but I don’t see how to use the half reaction method when there is

• ### Chemistry

Write the balanced equation for (aq) Pb(ClO3)2 and (aq) NaI. Include phases. What mass of precipitate will form if 1.50 L of concentrated Pb(ClO3)2 is mixed with .250 L of .110 M NaI? Assume the reaction goes to completion.

• ### chemistry

How do I balance a redox reaction for NaI + H2SO4 = H2S + I2 + Na2SO4 + H2O? I don’t understand how to balance the electron loss for Iodine.

• ### Chemistry

For a particular redox reaction NO2– is oxidized to NO3– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in basic solution. Phases are optional.

• ### chemistry

5.00g aluminum sulfide and 10.0g water react according to the reaction: Al2S3 + 6 H2O -> 2 Al(OH)3 + 3 H2S What is maximum mass of H2S that can be formed? What mass of excess reactant remains when the reaction is complete?

• ### chemistry

Consider the following balanced thermochemical equation for a reaction sometimes used for H2S production: 1/8 S8 (s) + H2 (g) ¨ H2S (g) ƒ¢Hrxn = -20.2 kJ (a)Is this an exothermic or endothermic reaction? (b)What is ƒ¢Hrxn for the reverse reaction?

• ### chemistry

In many residential water systems, the aqueous Fe3+ concentration is high enough to stain sinks and turn drinking water light brown. The iron content is analyzed by first reducing the Fe3+ to Fe2+ and then titrating with MnO4- in acidic solution. Fe2+(aq)

• ### chemistry-balanced redox equations

Use the following steps to balance the redox reaction below: Mg + Au+ Mg2+ + Au a. Write the oxidation and reduction half-reactions. Make sure each half-reaction is balanced for number of atoms and charge b. Multiply each half-reaction by the correct

• ### chemistry

Balance the following redox reaction by inserting the appropriate coefficients. H^+ +CrO4^2- +NO 2^- =Cr^3+ +H2O+NO3^-

• ### Analytic Chemistry

At 25 °C, you conduct a titration of 15.00 mL of a 0.0260 M AgNO3 solution with a 0.0130 M NaI solution within the following cell: Saturated Calomel Electrode || Titration Solution | Ag (s) For the cell as written, what is the voltage after the addition

• ## chemistry

H2O2 + KI = I2 + KOH IS this correct for a redox reactions? what does H2SO4 + Sugar turn into? from a redox reaction standpoint?

• ### Chem30

Balance the following redox reations: K2Cr2O7 + Nal + H2SO4 — Cr2(SO4)3 + I2 + H2O + Na2SO4 + K2SO4

• ### chemistry

Balance the following redox reaction using the half reaction method: NaIO3+KI==> I2+H20+Na(+1)+K(+1)

• ### Chemistry

in a particular redox reaction, Cr is oxidized to CrO42- and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in acidic solution.

• ### Chemistry

Label the following reactions as combination, decomposition, displacement, precipitation, or acid-base reaction. Also whether each reaction is a redox or non redox reaction. SO2(g)+H2O(l)-> H2SO3(aq) NH3(aq)+HS(-)(aq)-> NH4(+)(aq)+S(2-) Na2O2(l)->

• ### chemistry

Using the change-in-oxidation-number method, balance the redox reaction below. Show your work; partial credit will be given. NO2– + MnO4– → NO3– + Mn2+ Figure out which atoms’ oxidation numbers are changing, and by how much. Balance the equation

• ### chemistry

Using the half-reaction method, balance the redox reaction below. Show your work; partial credit will be given. I- + Br2 → IO3- + Br- Write the reduction and oxidation half-reactions. Balance them for atoms. Balance each of the half-reactions for charge.

• ### chemistry

Use the following steps to balance the redox reaction below: Mg + Au+ Mg2+ + Au -Write the oxidation and reduction half-reactions. Make sure each half-reaction is balanced for number of atoms and charge. -Multiply each half-reaction by the correct number,

• ### chemistry

Balance redox reaction. Fe(s) + O2(g) + H2O(l)–>Fe2+(aq) +OH-

• ### Chemistry

Consider the following reaction and select the false statement below. NaI + 3HOCl → NaIO3 + 3HCl A. HOCl is the oxidizing agent B. Cl is reduced C. NaI is the reducing agent D. If ΔG° for the reaction is < 0, then NaI is a stronger reducing agent than

• ### Chemistry

Help please, What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.350g of pure H2s(g), at 25 ∘C to achieve equilibrium? Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the

• ### Chem

Balance the following redox reactions in acidic solution by the half-reaction method Br–(aq) + I–(aq) + HClO(aq) = Br2(l) + IO3 + Cl–(aq)

• ### chemistry

please help this equation is driving my crazy. balance the following redox reaction in basic solution. H2O2 + ClO2 –> ClO-2 + O2

• ### chemistry

In a particular redox reaction, Cr is oxidized to CrO42– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in acidic solution. Phases are optional. Cr + Cu2+ = CrO42- + Cu+

• ### chemistry

Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s)⇌NH3(g)+H2S(g) This reaction has a Kp value of 0.120 at 25 ∘C. An empty 5.00-L flask is charged with 0.350 g of pure H2S(g), at 25 ∘C. What is the

• ### chemistry

balance the following redox equation. hno2(aq) + h2so4(aq) + k2cr2o7(aq)= hno3(aq) + cr2(so4)3 + h20 + k2s04

• ### Chemistry

What volume of each solution contains 0.220mol of NaI? a.) 0.142M NaI b.) 0.902M NaI c.) 1.61M NaI

• ### Chemistry

Balance the following redox equation using the oxidation-number-change method. Describe each step you use to balance the reaction. HCl(aq) + Zn(s) –> ZnCl2(s) + H2(g) I am really confused on how to do this as my book is very vague on this subject. Any

• ### chemistry

Ammonium bisulfide, NH2HS, forms ammonia NH3, and hydrogen sulfide, H2S through the reaction: NH4HS (s) NH3(g) + H2S(g) Kp value of .120 at 25C in a 5L flask is charged with .300g of H2S at 25C. A) What are the partial pressures of NH3 and H2S at

• ### Chemistry

Balance Redox using reactions by the 1/2 reaction method. NaIO3 (aq) + KI (aq) –>„³ I2 (s)

• ### AP Chemistry

redox reaction: Hydrogen peroxide is added to an acidified solution of potassium permanganate. what is the total redox reaction?

• ### science

AgNO3+NaCL=AgCL+NaNO3 is not a redox reaction but Cu+2AgNO3=2Ag+Cu(NO3)2 is a redox reaction.explain

• ### Chemistry

How would you balance this redox reaction by oxidation number method? C + O2 = CO2

• ### Chemistry Redox Reaction

Balance the equation as a redox reaction in acidic solution. Cu(s)+NO3^-1(aq)–>Cu^2+(aq)+NO(g)

• ### Chemistry 12

a) Use the standard reduction potentials table to balance the following redox equation: H2O2 + I + H = H2O + I2 b) Balance the following redox equation by the oxidation number method: Ag + HNO3 = AgNO3 + NO + H2O

• ### chemistry

balance the equations 1)Mg3N2+N2+H2O=Mg(OH)2+NH3 2)KMnO4+H2S+H2SO4=KHSO4+H2O+MnSO4

3)AS2O3+SnCl2+HCL=SnCl4+AS+H2O

• ### Chemistry

Balance the following redox reaction in acidic solution: H3PO4 + HNO2–> N2O4 + H3PO3

• ### Chemistry

For the following reaction, the equilibrium constant Kc = 97.0 at 900K. If the initial concentrations of NH3 and H2S are both 0.20 M, what is the equilibrium concentration of H2S? H2S(g) + NH3(g) = NH4HS(s) Would you have to create an ICE chart for this

• ### CHEMISTRY

BALANCE THE REDOX REACTION USING HALF CELL METHOD IN AN ACIDIC MEDIUM CHCl3 + MnO4- = Cl2 + CO2 + Mn+2

• ### science

determine if each equation represent a redox reaction.if it is a redox reaction, write dowm the two half reactions of(1) 2KCL3=2KCL+3O2,,(2)BaCL2+2KIO3=Ba(IO3)2+2KCL and (3)HCL+NaOH=H2O+NaCL

• ### chemistry

Balance each of the following redox equations using the half-reaction method. HI(s) + H2SO4 (aq) –> H2S(g) + I2 (s) My only question about this equation is…how do I know how many electrons I need to put on both sides? Other than that I know how to do

• ### Chemistry

I know nothing about chemistry, but am wondering if someone could help me with these. 1) Balance this redox reaction using the oxidation-number method. Zn + O2 + HCl ® ZnCl2 + H2O 2) Balance this redox reaction using the half-reaction method. (basic

• ### General Chemistry

Balance the following redox reaction in acidic and basic solutions: Fe(OH)2(s) + O2(g) –> Fe(OH)3(s) These are the steps my instructor gave us to balance redox reactions: 1. Divide into 1/2 rxns (reduction & oxidation) 2. Balance atoms other than H & O 3.

• ### Chemistry

1) Balance this redox reaction using the oxidation-number method. Zn + O2 + HCl ® ZnCl2 + H2O 2) Balance this redox reaction using the half-reaction method. (basic solution) Zn + MnO4- ® Zn(OH)2 + MnO2

• ### chemestry

PLEASE,COULD ANYONE HELP ME to balance this redox reaction : Cr2S3 PbO2 + H2SO4 + ——-> PbSO4 H2Cr2O7+H20

• ### Chemistry

Balanced equations done? Is each reaction a redox reaction? For those reactions that are redox reactions, I must identify the substance being oxidized and the substance being reduced… (a) Zn(s) + CoCl2 (aq) —> ZnCl2 (aq) + Co(s) (b) HI(aq) + NaOH(aq)

7.) How many moles of fluroine are required to react with 12 g of sodium iodide? I already balanced it but am confused to go from here F2 + 2 NAi —- 2 NaF + I2 12 g NaI + 2 mol NAI/149.89 gNAi * 1 mol NAF/1 mol NAi * 1 mol F2 / 2 mol NaF 1.) how many

• ### chemistry

how do u do a redox balance of the following reaction : Fe(NH4)2(SO4)2*6H2O + H2C2O4 + K2C2O4 + H2O2 -> K3Fe(C2O4)3*3 H2O + (NH4)2SO4 + H2SO4 +H2O i only know Fe2+ -> Fe3+ +1e-

• ### chemistry

Can anyone give me a brief explanation about redox? I’m just not understanding any of it. How do you know if a reaction is redox or non redox….how do you know what would be reduced? I am just confused with the redox subject. Any direction?

• ### Chemistry

Balance the equation: _MnO4– + _H+ + _Fe2+ => _Mn2+ + _H2O + _Fe3+ How do you do balance this redox reaction?

• ### Chem30

Balance the following redox reations: K2Cr2O7 + Nal + H2SO4 — Cr2(SO4)3 + I2 + H2O + Na2SO4 + K2SO4

• ### chemistry

Balance the following redox equation. hno2(aq) + h2so4(aq) + k2cr2o7(aq)= hno3(aq) + cr2(so4)3 + h20 + k2s04?

• ### chemistry

Complete and balance the chemical equation using compound formulas. Include the states. If there is no reaction, enter NR. Pb(NO3)2(aq) + NaI(aq) → sine Pb is not reactive, the reaction is NR. Am i correct?

• ### chemistry

Heterogenous equilibrium of ammonium bisulfide. Ammonium bisulfide NH4HS forms ammonia NH3 and hydrogen sulfide H2S through the reaction NH4HS(s) arrows + H2S(g). This reaction has a kp value of 0.120 at 25 C. A 5.0-L flask is charged with .400g of pure

• ### Chemistry

Hi, I was given the reactants for the chemical reaction and I am supposed to write the product. The equation must be balanced. Can someboy please check my work? Thanks 🙂 3NaOH + Fe(NO3)3 –> Fe(OH)3 + 3Na(NO3) 2NH3 –> N2 + 3H2 2H2 + o2 –> 2H2O 4Mg +

• ### Chemistry

Balance the redox reaction below using the half-reaction method. Bi3+(aq) + Co(s)Bi(s) + Co2+(aq)

• ### AP CHEMISTRY

A mixture of H2, S, and H2S is held in a 1.0-L vessel at 90°C and reacts according to the equation H2(g) + S(s) H2S(g). At equilibrium the mixture contains 0.46 g of H2S and 0.40 g H2. (a) Write the equilibrium-constant expression for this reaction (Kc).

• ### Chemistry

Balance the redox reaction: Ag(aq)+Cu(s)= Ag(s)+Cu(aq)

• ### Chemsitry

For a particular redox reaction NO2– is oxidized to NO3– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in basic solution. Phases are optional.

• ### Chemistry

The reaction between 0.045 g of calcium with an excess of water was carried out in an ice calorimeter as used in this lab. The volume of water in the calorimeter decreased by 0.18 mL during the reaction a) Write the equation for the reaction which occurs.

• ### chemistry

O3SOOSO3^(2−) + Cr^(3+)+ -> HSO4^(1-) + Cr2O7^(2-). Could someone balance this redox reaction for me? I can’t figure it out. Thanks

• ### Chemistry

I’m supposed to balance a redox reaction that occurs in an acidic solution. I already balanced it(h**p://img148.imageshack.us/img148/4304/redoxht8.jpg), but how do I tell if a half-reaction is oxidation or reduction? I know an oxidation reaction loses

• ### chemistry

For a particular redox reaction NO is oxidized to NO3^– and Cu^2+ is reduced to Cu. Complete and balance the equation for this reaction in basic solution: NO + Cu^2+ –> NO3^- + Cu^+ help. thanks.

• ### chemistry

Please, will someone help me balance this equation? There’s always one element I just can’t seem to balance. Cu+HNO3===>NO2+Cu(NO3)2+H20 Thanks for the help. Try this. Cu + 4HNO3 ==> 2NO2 + Cu(NO3)2 + 2H2O You’re a genius! Do you think you could tell me

• ### Chemistry

Consider the reaction: 2 H2S(g)–>

• ### Chemistry

Consider the reaction: 2 H2S(g)–>

• ### Chemistry

Balance the redox reaction.2NaClO3+4HCl-2ClO2+2H2O+2NaCl+Cl2

• ### Chemistry

Mno4 + fe2 —-> mn2 + fe3 Balance the redox reaction in acidic medium

• ### chemistry

Ag+HNO3—–AgNO3+NO+H2O balance the redox reaction using the oxidation-number method

• ### Chemistry

Balance the following redox reaction in acidic solution: H3PO4 + HNO2–> N2O4 + H3PO3

• ### Chemistry

Balance the following redox reaction in acidic solution: H3PO4 + HNO2–> N2O4 + H3PO3

• ### Chemistry

Please check this over and see of they are right…if they are not can you please tell the the right answer and explain how you got it. I think I am getting myself confused. Thank you. Write the neutralization reaction for each of the following. Balance

• ### Chemistry

1.A description of fuel cells of redox reactions, including a description of the product or procedure that the redox reaction is used in, and what are the products and reactants of the redox reactions. 2.The benefits of using electrochemical processes and

• ### Chemistry

For the following reaction, the equilibrium constant KC = 97.0 at 900 K. If the initial concentrations of NH3 and H2S are both 0.20 M, what is the equilibrium concentration of H2S? H2S (g) + NH3 (g) —> NH4HS (s)

• ### Chemistry

For the following reaction, the equilibrium constant KC = 97.0 at 900 K. If the initial concentrations of NH3 and H2S are both 0.20 M, what is the equilibrium concentration of H2S? H2S (g) + NH3 (g) —> NH4HS (s)

• ### chem for Dr. Bob

In the reaction 2 H2(g) + S2(g) reverse reaction arrow 2 H2S(g), Kc = 6.28 multiplied by 103 at 900 K. What is the equilibrium value of [H2] if at equilibrium [H2S] = [S2]1/2?

Above are some summary of question to help you learn more and review the equation and find some way to resolve the homework. Bpackingapp.com wish you have a

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