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- . To obtain useful electrical energy from an oxidation-reduction process, we must set up the reaction in such a way that the Oxidation half-reaction and the reduction half-reaction are physically one _____another.In the balanced oxidation-reduction reaction (occurring in acidic condition) the coefficients before H^+ and SO3^2- are __ and __, respectively? SO3^2- + NO3^¯ → NH4^+ + SO4^2-cyanate ion in waste solutions from gold mining operations can be destroyed by treatment with hypochlorite ion in basic solution. write a balanced oxidationp-reduction equation for this reaction OCN-(aq) + OCI-(aq) + OH-(aq) --> CO32-(aq) + N2(g) + Cl-(aq) + H2O(l) hint: notice that in the oxidation of half-reaction, OCN- yields to two products
- consider the redox reaction 5Fe^+2 (aq) + MnO4- (aq) +8H+ (aq) ---> 5Fe^+3 (aq) + Mn^+2 (aq) + 4H2O A 15.00 mL volume of 0.1650 M KMnO4 solution is needed to oxidize 25.00 mL of a FeSO4 solution in acidic medium. WHat is the concentration of the FeSO4 solution in molarity?MnO4- can be used in a redox titration to determine the amount of H2C2O4 in an unknown sample. Below is an unbalanced reaction that describes this process: MnO4- + H2C2O4 --> Mn2+ + CO2 25.00 mL of a solution containing an unknown amount of H2C2O4 (MW = 90.03 g/mol) required 18.31 mL of 0.1153 M MnO4- to react completely. Calculate the molarity of the original unknown H2C2O4 solution.NOTE: This is a redox titration, so remember to balance each half reaction and then add them together to arrive at the overall balanced reaction. To help you out, I will tell you that each C in H2C2O4 has a 3+ charge. Also, if your overall balanced reaction doesn't have 8 waters on the right, you have done something incorrectly.Oxidation /reduction reactionsWhich of the following are oxidation-reduction reactions? Place a (*)to the LEFT of those satisfying this criterion. To the RIGHT of each equation, give the HIGHEST oxidation number and the species to which it is associated. Thus, a correct answer might appear as: Sample: * 2 N2O5(g)→ 4NO2(g) + O2(g) [N5+] a. 2Na + Cl2→ 2NaCl b. C + O2→ CO2 c. 2H2O 2H2 + O2 d. NaCl + AgNO3→ AgCl + NaNO3 e. NH3 + HCl → NH4+1 + Cl-1 f. 2KClO3→ 2KCl + O2 g. H2 + Cl2→ 2HCl h. 2H2 + O2→ 2H2O i. H2SO4 + 2KOH →K2SO4 + 2H2O j. Zn + CuSO4→ZnSO4 + Cu
- A sample of impure tin of mass 0.535 g is dissolved in strong acidto give a solution of Sn2+. The solution is then titrated with a0.0448 M solution of NO3-, which is reduced to NO(g). Theequivalence point is reached upon the addition of 0.0344 L of theNO3- solution. Find the percent by mass of tin in the originalsample, assuming that it contains no other reducing agents.(A) if both sentences are true,(B) if both sentences are false,(C) if the first sentence is true but the second is false, and(D) if the first sentence is false but the second is true. 1. An acidic and a basic solution may be used to balance the redox reaction when the oxidation number method is employed. The final step in balancing redox reactions using the oxidation number method is to balance by inspection. 2. In the oxidation number method of balancing redox reactions, there is a need to add water and hydroxide ions on both sides of the chemical reaction. The oxidation state of oxygen is always (-2) except for peroxides. 3. In the half-reaction method of balancing redox reactions, the reaction is divided into three half-reactions. In a redox reaction, the oxidation number of iron changed from +2 to +3; thus, sulfur is an oxidizing agent. 4. In a redox reaction, the oxidation number of iron changed from +2 to +3; thus, sulfur is a reducing agent. In a redox reaction, the oxidation…The following skeletal oxidation-reduction reaction occurs under basic conditions. Write the balanced OXIDATION half reaction. Hg + HPbO2- ----->HgO + Pb __________ ---> _____________ Reactants. Products.
- Place the stoichiometric coefficient for each of the following species in the properly-balanced redox equation that takes place in acidic solution below (Please include coefficients of either "0" or "1" as appropriate. BiO3- (aq) + Mn2+ (aq) --> MnO4- (aq) + Bi3+ (aq) We are to balance this equation by using 1/2 reactions and build from the based on adding H+, H20, and charges. If this could be shown in detail I would greatly appreciate it! This is the work that I have done so far...When the following skeletal equation is balanced under acidic conditions, what are the coefficients of the species shown?Mg2+ + NO ----> Mg + HNO3Water appears in the balanced equation as a (reactant, product, neither) with a coefficient of . (Enter 0 for neither.) What species is the reducing agent?When the following half reaction is balanced under basic conditions, what are the coefficients of the species shown? ____P + ____ H2O-----> ____ PH3 + ____ OH-In the above half reaction, the oxidation state of phosphorus changes from ___ to____ .