Chemistry, 30.08.2019 00:30, abdominguez7307

What is added to balance hydrogen and oxygen atoms in an oxidation reduction reaction in acidic solution?

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Chemistry, 31.07.2019 10:30, UsedForSchool2018

Me in the oxidation part of an oxidation-reduction reaction, the substance undergoing oxidation: loses electrons gains electrons shares electrons combines protons if any of the reactants or products in a reaction contains oxygen, then the reaction is a redox reaction. true preventing iron corrosion is important because many structures, including bridges and iron railings, are likely to rust over time and become weaker. which of the following conditions would make corrosion more likely? increasing the moisture level near the reducing the concentration of electrolytes in solutions in contact with the structure neutralizing any acidic solutions near the iron painting the iron surface the oxidation number of a metal is always the same for that metal. true the sum of all oxidation numbers: in a neutral molecule = 0 in an ion = a + in an ion = the charges on neutral atoms do not need to be equal on both sides of a chemical equation in the reaction, 2 li (s) + cl2 (g) imported asset 2 licl (s), the reducing agent is: the the cl2 the licl both the li and the cl2 in the reaction, c + 2 s imported asset cs2, the substance that is the oxidizing agent is: the c the the cs2 both the c and the s how many electrons should be added to balance the following oxidation half-reaction, h2o2 imported asset 2 h+ + o2? none one four when balancing the oxidation and reduction half-reactions for acidic solutions, you should: use h+ and oh− equally in order to balance the use h+ only in order to balance the equation use h+ and h2o, as needed to balance the equation use oh− and h2o, as needed to balance the equation the half-reaction occurring at the anode of an electrochemical reaction is comparable to: the oxidation portion of a reaction in a redox the reduction portion of a reaction in a redox reaction both the oxidation and the reduction portions of the redox reaction, at various times the unbalanced portion of either side of a redox equation the voltaic cell produces electric current from a spontaneous chemical reaction, but electrolytic reactions are not spontaneous. false

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Chemistry, 08.08.2019 04:20, JulietteRosso995

One method for determining the concentration of hydrogen peroxide in solution is through a redox titration with potassium permanganate under acidic conditions. in this procedure the hydrogen peroxide reduces the permanganate ion. a. what is the oxidation number of the mn ion in the potassium permanganate? 3. b. write the balanced half reaction for permanganate ion to form mn2* in the acidic solution. c. write the balanced half reaction for hydrogen peroxide in the acidic solution in which oxygen gas is released. d. write the balanced complete reaction. e. in a titration of a 100.0-ml hydrogen peroxide solution, the analyte turned a faint pink after the addition of 3.56 ml of a 0.30 m potassium permanganate solution what is the concentration of the hydrogen peroxide in the solution?

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Chemistry, 18.09.2019 18:30, SoccerHalo

Balance the oxidation-reduction reaction presented below using the half-reaction method. the reaction occurs in acidic solution. cr2o72- (aq) + ci+ (aq) → cr3+ (aq) + cl2 (g)

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Chemistry, 06.10.2019 12:00, cmob13

Which of the following is not a step in balancing redox reactions in acidic solution, using the half-reaction method? a) h2o and oh- are added as needed to the half-reaction equations to make the number of oxygen and hydrogen atoms balance. b) divide the chemical equation into two half-reaction equations, identifying which half-reaction is oxidation and which is reduction. c) h2o and h+ are added as needed to the half-reaction equations to make the number of oxygen and hydrogen atoms balance. d) multiply each term in one of the half-reaction equations by a factor that will make the number of electrons lost (in the oxidation) equal to the number of electrons gained (in the reduction).

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