Why must the charge balance in oxidation-reduction reactions?

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queen_honey_blossom answered 2 years ago

In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons...

In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reaction method or the oxidation number method. The half-reaction method balances the electrons lost in the oxidation half-reaction with the electrons gained in the reduction half-reaction. In either method H2O(l), OH?(aq), and H+(aq) may be added to complete the mass balance. Which...

Redox (oxidation-reduction) reactions in glycolysis

Part A - Redox (oxidation-reduction) reactions in glycolysis In glycolysis, as in all the stages of cellular respiration, the transfer of electrons from electron donors to electron acceptors plays a critical role in the overall conversion of the energy in foods to energy in ATP. These reactions involving electron transfers are known as oxidation-reduction, or redox, reactions. Drag the words on the left to the appropriate blanks on the right to complete the sentences. 1. When a compound donates (loses)...

What is Oxidation-reduction reactions? What is FDA ?

What is Oxidation-reduction reactions What is FDA What is GRAS What is patent What is USDA

Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and...

Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and label each accordingly. Give the complete balanced reaction. A.) CN-1 + MnO4-2 ---> CNO-1 + MnO2 B.) S2O3-2 + IO2-1 ---> I- + S4O6-2

Use the half reaction method to balance each of the following oxidation-reduction reactions. Identify the oxidizing...

Use the half reaction method to balance each of the following oxidation-reduction reactions. Identify the oxidizing agent and the reducing agent. A) Cu(s) + Ag+(aq) ---> Ag(s) + Cu2+ B) Al(s) + I2(s) ---> AlI3(s) C) Pb(s) + Fe3+(aq) ----> Pb2+(aq) + Fe(s)

balance each of the following oxidation/reduction reactions utilizing the half reaction method, H2O2 (aq) + Cl2O7...

balance each of the following oxidation/reduction reactions utilizing the half reaction method, H2O2 (aq) + Cl2O7 (aq) → ClO2- (aq) + O2 (g) in basic solution

In an acid solution using the half-reaction method balance the following oxidation/reduction reactions. Identify the oxidizing...

In an acid solution using the half-reaction method balance the following oxidation/reduction reactions. Identify the oxidizing agent and the reducing agent in each reaction. a. ??(?) + ??3 - (??) → ??2+ (??) + ??(?) b. ??2?72-(??) + ??-(??) → ??3+(??) + ??2 (?) c. ??22+(??) + ??(?) → ?4+(??) + ???42- d. ??2 (??) → ???3-(??) + ??-(??)

1. Balance the following oxidation-reduction reactions using the half-reaction method and tell the number of electrons...

1. Balance the following oxidation-reduction reactions using the half-reaction method and tell the number of electrons transferred in the balanced oxidation-reduction reaction a) S2-(aq) + NO3-(aq) ---> S8(s) + NO2(g) acidic solution b) MnO4-(aq) + I-(aq) ---> MnO2(s) + IO3-(aq) basic solution c) Sb(s) + H2SO4(aq) ---> Sb2(SO4)3(s) + SO2(g) acidic solution d) H2O2(aq) + MnO4-(aq) ---> MnO2(s) + O2(g) basic solution

Oxidation states are important for keeping track of electrons in oxidation-reduction reactions. Here are some general...

Oxidation states are important for keeping track of electrons in oxidation-reduction reactions. Here are some general rules to remember: In most cases, oxygen has an oxidation state of −2. Group 1 and group 2 elements on the periodic table have +1 and +2 oxidation states, respectively. In most cases, hydrogen has an oxidation state of +1. Many elements can have more than one oxidation state. In such cases, use the other elements in the compound whose oxidation states are known...

Balance the following oxidation–reduction equation. The reactions occur in a basic aqueous solution. Cd2++ H 2S → Cd...

Balance the following oxidation–reduction equation. The reactions occur in a basic aqueous solution. Cd2++ H 2S → Cd + S 8 S2- + F2 → SO42- + F- Cr + NO3- → Cr(OH)4- + NH3 MnO4- + C2O42- → MnO2 + CO2

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