1. Define oxidation numberm oxidation, reduction, reducing agent and oxidizing agent. 2. What is oxidized and what is reduced in the following reaction: N2 + 202 → 2NO2

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SCH4U1
Assignment 5
1. Define oxidation numberm oxidation, reduction, reducing agent and oxidizing agent.
2. What is oxidized and what is reduced in the following reaction: N2 + 202→ 2NO2
3. Determine the oxidation number of each element in the following substances:
a ) H2SO4
d ) KMNO4
b) Ca3(PO4)2
e ) H3ASO4
с) Clz
f) CaSnO3
4. Balance the following equations (use the oxidation number method):
a) MnO4¯ + Fe
b) HNO3 + H;S
c) Cr2O,²- + ci~
d) Cr(OH)3(s) + ClO;'(aq)
Mn?* + Fe* (acidic solution)
NO + S
+ Cl2 (acidic solution)
CrO2 (aq) + Cl'(aq) (basic solution)
5. Iodine normally has oxidation numbers of -1 and 0. Could I2 serve as a reducing agent?
Explain why or why not.
6. Describe what happens when chlorine in water is mixed with bromide ions and cyclohexane (a
non-polar solvent). Explain why this happens.
7. Should chlorine gas be passed through copper tubing? Explain your answer using Eº values.
8. Balance the following equations using the half-reaction method.
а) Ва (s) + CI,
b) Zn (s) + S0,- + H*
c) MnO4 + NO, + H2O
d)r + NO,¯ + H'
Ba* + CI
H,SO3 (g) + Zn²* + H,O
Mn* + NO, + H*
h + NO2 + H2O
9. For each set of reactants, write a redox equation for the reaction that may occur. Calculate the
E°cell values and determine if the reaction is spontaneous.
a) Mg(s) + A1³*
d) Sn(s) + H*
b) Hg** + Ag(s)
e) H2(g) + C12(g)
c) CI + ½(s)
) Cu(s) + I
10. Name two substances which oxidize Ag to Ag*.
11. Draw the following galvanic (voltaic) cells (salt bridge design) and label the following:
i) anode and cathode
ii) oxidation and reduction half reaction
iii) direction of electron, cation and anion movement
iv) net reaction
v) calculate the E cll
a) Co«) |Co(NO3)2 (aq) || Zn(NO3)2 (aq) | Zn (s) (standard conditions)
b) Au(s) |Au(NO;); (aq) || H2(g), HCI (aq) | Pt (s) (hydrogen standard cell)
c) Sn(s) |Sn{NO3))2 (1.00 M) || Zn(NO)2 (0.0100 M) | Zn(s)
Transcribed Image Text:SCH4U1 Assignment 5 1. Define oxidation numberm oxidation, reduction, reducing agent and oxidizing agent. 2. What is oxidized and what is reduced in the following reaction: N2 + 202→ 2NO2 3. Determine the oxidation number of each element in the following substances: a ) H2SO4 d ) KMNO4 b) Ca3(PO4)2 e ) H3ASO4 с) Clz f) CaSnO3 4. Balance the following equations (use the oxidation number method): a) MnO4¯ + Fe b) HNO3 + H;S c) Cr2O,²- + ci~ d) Cr(OH)3(s) + ClO;'(aq) Mn?* + Fe* (acidic solution) NO + S + Cl2 (acidic solution) CrO2 (aq) + Cl'(aq) (basic solution) 5. Iodine normally has oxidation numbers of -1 and 0. Could I2 serve as a reducing agent? Explain why or why not. 6. Describe what happens when chlorine in water is mixed with bromide ions and cyclohexane (a non-polar solvent). Explain why this happens. 7. Should chlorine gas be passed through copper tubing? Explain your answer using Eº values. 8. Balance the following equations using the half-reaction method. а) Ва (s) + CI, b) Zn (s) + S0,- + H* c) MnO4 + NO, + H2O d)r + NO,¯ + H' Ba* + CI H,SO3 (g) + Zn²* + H,O Mn* + NO, + H* h + NO2 + H2O 9. For each set of reactants, write a redox equation for the reaction that may occur. Calculate the E°cell values and determine if the reaction is spontaneous. a) Mg(s) + A1³* d) Sn(s) + H* b) Hg** + Ag(s) e) H2(g) + C12(g) c) CI + ½(s) ) Cu(s) + I 10. Name two substances which oxidize Ag to Ag*. 11. Draw the following galvanic (voltaic) cells (salt bridge design) and label the following: i) anode and cathode ii) oxidation and reduction half reaction iii) direction of electron, cation and anion movement iv) net reaction v) calculate the E cll a) Co«) |Co(NO3)2 (aq) || Zn(NO3)2 (aq) | Zn (s) (standard conditions) b) Au(s) |Au(NO;); (aq) || H2(g), HCI (aq) | Pt (s) (hydrogen standard cell) c) Sn(s) |Sn{NO3))2 (1.00 M) || Zn(NO)2 (0.0100 M) | Zn(s)
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