Write a balanced half-reaction for the reduction of permanganate ion, MnO-4, to

Question

Write a balanced half-reaction for the reduction of permanganate ion, MnO-4, to MnO2 in a basic solution, Mn04-(aq) + 4 OH(aq) + 3 e- rightarrow MnO2(s) + 2 H2O( lambda ) + 2 O2(g) MnO4-(aq) + 2 OH (aq) + 3 e- rightarrow MnO2(s) + 2 HO2(aq) MnO4-(aq) + 3 e+ rightarrow MnO2(s) + O2(g) MnO4-(aq) + 2 H+(aq) + 3 e- rightarrow Mn02(s) + 2 OH-(aq) MnO4-(aq) + 2 H2O( lambda ) + 3 e- rightarrow MnO2(s) + 4 OH-(aq) Write a balanced chemical equation for the following reaction in an acidic solution. Cr2O72-(aq) + Br(aq) rightarrow Cr3+(aq) + Br2(aq) Cr2O72-(aq) + 2 Br-(aq) rightarrow 2 Cr3+(aq) + Br2(aq) Cr2O72-(aq) + 6 Br-(aq) + 14 H+(aq) rightarrow 3 Br2(aq) + 2 Cr3+(aq) + 7 H2O( lambda ) Cr2O72-(aq) + 2 Br-(aq) + 14 H+(aq) rightarrow 2 Cr3+(aq) + Br2(aq) + 7 H2O( lambda ) Cr2O72-(aq) + 2 Br-(aq) + 7 H+(aq) rightarrow 2 Cr3+(aq) + Br2(aq) + 7 OH-(aq) Cr2O72-(aq) + 6 Br-(aq) + 7 H+(aq) rightarrow 2 Cr3+(aq) + 3 Br2(aq) + 7 OH-(aq) Write a balanced chemical equation for the following reaction in a basic solution. CI03-(aq) + MnCOHMs) rightarrow Cl-(aq) + MnO2(s) 2 C1O3-(aq) + Mn(OH)2(s) rightarrow 2 Cl-(aq) + MnO2(s) + 2 H2O( lambda ) + 2 O2(g) 2 C1O3-(aq) + 3 Mn(OH)2(s) rightarrow 2 Cl-(aq) + 3 MnO2(s) + 6 OH-(aq) 2 C1O3-(aq) + 3 Mn(OH)2(s) + 6H+(aq) rightarrow 2 Cl-(aq) + 3 MnO2(s) + 6 H2O( lambda ) C1O3-(aq) + 3 Mn(OH)2(s) rightarrow Cl-(aq) + 3 MnO2(s) + 3 H2O( lambda ) C1O3-(aq) + 2 Mn(OH)2(s) rightarrow Cl-(aq) + 2 MnO2(s) + 2 OH (aq) + H20( lambda ) All of the following statements concerning voltaic cells are true EXCEPT a salt bridge allows cations and anions to move between the half-cells. electrons flow from the cathode to the anode. reduction occurs at the cathode. a voltaic cell can be used as a source of energy. a voltaic cell consists of two-half cells. What is the correct cell notation for a voltaic cell based on the reaction below? Ni2+(aq) + Zn(s) rightarrow Ni(s) + Zn2*(aq) Zn(s) | Zn2+(aq) || Ni2+(aq) | Ni(s) Zn(s) || Zn2+(aq), Ni2+(aq) | Ni(s) Ni(s) || Ni2+(aq), Zn2l-(aq) || Zn(s) Ni(s) | Zn2+(aq) || Ni2+(aq) | Zn(s) Ni(s) | Ni2+(aq) || Zn2+(aq) | Zn(s)

Explanation / Answer

6) d
7) c
8) d
9) b. (electrons always flow from anode to cathode)

10) a

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