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Calculate E° for the reaction: 4 As + 3 O2 + 2 H2O →4 HAsO2 E°O2/H2O, H3O+ = +1.229, E°HAsO2/As, H3O+ = +0.248 Round your answer to 3 significant figures. V The number of significant digits is set to 3; the tolerance is +/-4%
Balance the following redox reactions: a) CN− + MnO4− → CNO− + MnO2 (basic solution) b) O2 + As → HAsO2 + H2O (acidic solution) c) Br− + MnO4− → MnO2 + BrO3− (basic solution) d) NO2 → NO3− + NO (acidic solution) e) ClO4− + Cl− → ClO− + Cl2 (acidic solution) f) AlH4− + H2CO → Al3+ + CH3OH (basic solution)
Balance Redox reactions (show step wise process) FeS2 + O2 + H2O → Fe2+ + SO42- + H+
Balance the following redox reactions: Fe^2+ + MnO4^- + H^+ → Fe^3+ + Mn^2+ + H2O Mn^2+ + MnO4^- + …→ MnO2 + … IO3^- + I^- + H^+ → I2 + H2O
Which of the following are redox reactions? (select all that apply) S8 + O2 → SO3 NaBr + CaF2 → NaF + CaBr2 C3H6 + O2 → CO2 + H2O Mg + Cl2 → MgCl2
Split the following unbalanced redox reactions into a reduction half-reaction and an oxidation half-reaction. Balance both the elements and the number of electrons. a) Fe(3+) + Cu --> Fe(2+) + Cu(2+) b) CH4 + O2 --> CO2 + H2O
Determine the products of the following reactions. After, balance them: a) Fe2(SO4)3 + H2O + SO2 + KMnO4 = b) Fe2(SO4)3 + H2O + SO2 + KCr2O7 = c) Fe2(SO4)3 + H2O + SO2 + H2O2 = d) What would the above 3 reactions look like if you added KSCN? Write the balanced equations for them. *these were all apart of a chem lab in order to detect the presence of Fe+2 ions* *these are redox reactions*
Balance the following redox reactions. Show the electron exchange for the species involved in the redox process. (4 reactions x 5 pts. each = 20 pts. total) 1. KCIO → KCIO. + KCI 2. CH,OH + KMnO4 + H2SO4 → HCOOH + K SO4 + MnSO4 + H2O 3. V20 + Ca + V + CaO We were unable to transcribe this image
Balance the following redox reactions by balancing the half reactions and then combine the half reactions to get the overall balanced redox reaction with the lowest possible whole number coefficients. 1. Consider the following unbalanced redox reaction: MnO2(s) + BrO3−(aq) → MnO4−(aq) + Br−(aq) (a) Balance the corresponding half reactions in acidic conditions using the lowest possible whole number coefficients. (Enter coefficients for one and zero. Blanks will be marked incorrect.) MnO2(s) + H2O(l) + OH−(aq) + H+(aq) + e− → MnO4−(aq) + H2O(l) + OH−(aq) + H+(aq)...
Balance each of the following redox reactions in basic solution. 18.34 Balance each of the following redox reactions in basic solution. (a) CIO-(aq) + CrO(aq) → C1- (aq) + Cro (aq) (b) Br2(aq) + Br (aq) + BrO3(aq) (c) H2O2(aq) + N H(aq) → N2(g) + H2O(O)