1. Determine the oxidation state for all elements in the following molecules 2. Complete the reduction and oxidation equation and write the redox equation in the following examples 3. Complete the equation and indicate the standard reduction potential Ered assuming both reac-tions partners are used in the same concentration. 4. Calculate E for the following redox pair

**Exercises**

**1.** **Determine the
oxidation state for all elements in the following molecules:**

(a)
H_{2}O

(b)
NaCl

(c)
H_{2}O_{2}

(d)
Fe_{2}O_{3}

(e)
MnO_{4}^{−}

(f)
Cr_{2}O_{7}^{2−}

(g)
SiH_{4}

**2. Complete
the reduction and oxidation equation and write the redox equation in the
following examples:**

(a) MnO_{4}^{−} + Fe^{2+}+
???? → Mn^{2+}
+ Fe^{3+}+ ?????? under acidic conditions

(b) MnO_{4}^{−} + Br^{−}
+ OH^{−} → ??? + BrO_{3}^{−} under basic conditions

(c) Cr_{2}O_{7}^{2−} +
Cu^{+} → Cu^{2+}+ ??? under acidic conditions

(d) IO_{3}^{−} + I^{−}
→ I_{2}
under acidic conditions

**3. Complete
the equation and indicate the standard reduction potential E _{red}
assuming both reac-tions partners are used in the same concentration.**

(a) Br_{2} + 2I^{−} → ???? *E*_{0}(Br_{2}∕Br^{−})
=* *1*.*07 V

*E*_{0}(I_{2}∕I^{−})
=* *0*.*54V

(b) Fe^{2+} + Ce^{4+} → ???? *E*_{0}(Ce^{4+}∕Ce^{3+})
=* *1*.*61 V

*E*_{0}(Fe^{3+}∕Fe^{2+})
=* *0*.*77 V

(c) Br_{2} + Fe → ???? *E*_{0}(Br_{2}∕Br )=107V

*E*_{0}(Fe^{2+}∕Fe)
= −0*.*44 V

**4. Calculate
E for the following redox pair when
Mn^{3}**

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