Practice with Half Reactions
For the following balanced redox reaction answer the following questions
Mg(s) + 2HCl (aq)  MgCl2 (aq) + H2 (g)
1.
a. What is the oxidation state of Mg (s)?
d. What element is reduced?
b. What is the oxidation state of Cl in HCl?
e. How many electrons are transferred?
c. What element is oxidized?
2 Fe+2(aq) + H2O2(aq)  2Fe+3(aq) + 2 OH-1(aq)
2.
a. What is the oxidation state of oxygen in
c. What is the element that is reduced?
H2O2?
b. What is the element that is oxidized?
d. How many electrons are transferred in the
reaction as it is balanced?
4NaOH(aq) + Ca(OH)2(aq) + C(s) + 4ClO2(g)  4NaClO2(aq) + CaCO3(s) + 3H2O(l)
3.
a. What is the oxidation state of Cl in ClO2(g)?
d. What is the element that is reduced?
b. What is the oxidation state of C in C(s)?
c.
What is the element that is oxidized?
e. How many electrons are transferred in the
reaction as it is balanced?
4. Which of the following equations does not represent an oxidation-reduction reaction?
A. 3Al + 6HCl  3H2 + AlCl3
B. 2H2O  2H2 + O2
C. 2NaCl + Pb(NO3)2  PbCl2 + 3NaNO3
D. 2NaI + Br2  2NaBr + I2
E. Cu(NO3)2 + Zn  Zn(NO3)2 + Cu