Chemistry
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Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Use the half-reaction method to balance the following equation in basic solution:
Fe2+ + MnO4
Fe+ + Mn2+ (Do not include the states of matter.)
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- Write a balanced overall reaction from these unbalanced half-reactions. Cu⟶Cu2+Cu⟶Cu2+ Ag+⟶Agarrow_forwardBalance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --arrow_forward10. Balance the following redox reaction using the half-reaction method and tell how many electrons are transferred in the reaction. Ag(s) + CN (aq) +O2 (g) → Ag(CN), + H2O (BASIC medium) HINT: CN- is neither oxidized nor reducedarrow_forward
- Balance the following redox reaction in basic solution. MnO4(aq) + Cl (aq) MnO₂ (s) + Cl₂(g)arrow_forwardFor Questions 11-16: Balance the following oxidation-reduction reaction in acidic conditions using the half reaction method by following the step described in each question. ??2?−27(??)+???2(??)⟶??+3(??)+??−3(??)Cr2O7−2(aq)+HNO2(aq)⟶Cr+3(aq)+NO3−(aq) Step 1: Assign the oxidation states of each ATOM in the reaction before and after the reaction takes place. Reactants: Cr = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] O = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] H = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] N = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] Products: Cr = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] O = ["", "", "", "", "", "",…arrow_forward
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