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Table J: Activity Series
which are less active.
• The higher the element on the chart, the more active the element is.
Na is more active than Cr, so it’s higher on the chart.
2H2(g) + O2(g) 2H2O(􏰀) Ti is less active than K, so it’s lower on the chart.
• The more active metals get oxidized more easily.
• The more active nonmetals get reduced more
easily.
There are many Regents questions based on this topic.
)
C(s) + O2(g) CO2(g)
6CO 2
22 2
2
2
g)
3CO
2H2(g) + O2(g) 2H2O(g)
g)
2
2C(s) + 3H2(g) C2H6(g)
2C(s) + 2H2(g) C2H4(g)
2C(s) + H2(g) C2H2(g) H2(g) + I2(g) 2HI(g)
2(g
Table I
Table J
Heats of Reaction at 101.3 kPa and 298 K
C
Activity Series**
Metals
Nonmetals
Li Rb K Cs Ba Sr Ca Na Mg Al Ti Mn Zn Cr Fe Co Ni Sn Pb H2 Cu Ag Au
F2 Cl2 Br2 I2
Reffy, Table J (p. 5) shows us which elements are more active and
Reaction ∆H (kJ)* CH4(g) + 2O2(g) CO2(g) + 2H2O(􏰀) –890.4
Most Active
Most Active
H
8(g)
+
5O 2(
2(g
3
2C8H18(􏰀) + 25O2(g) 16CO2(g) + 18H2O(􏰀) –10943 2CH3OH(􏰀) + 3O2(g) 2CO2(g) + 4H2O(􏰀) –1452 C2H5OH(􏰀) + 3O2(g) 2CO2(g) + 3H2O(􏰀) –1367
C6H 12O
(g)
less active the element is.
6(s
280
)+
2CO(g) + O2(g) 2CO2(g)
6O
4 –566.0 –393.5 –3351 +182.6 N (g) + 2O (g) 2NO (g) +66.4
)+
4
H2O
+ 6H 2
O
(􏰀
)
–2
(􏰀)
–
21
9.2
• The lower the element on the chart, theN (g) + O (g) 2NO(g)
4Al(s) + 3O2(g) 2Al2O3(s)
–483.6 –571.6 –91.8 –84.0 +52.4 +227.4 +53.0 +34.89 –44.51 +14.78 +25.69 +3.88 –48.83 H+(aq) + OH–(aq) H2O(􏰀) –55.8
*The ∆H values are based on molar quantities represented in the equations. A minus sign indicates an exothermic reaction.
N
(g) 223
+
3
H(
HO
KNO3(s) 2 K+(aq) + NO3–(aq)
NaOH(s) H2O Na+(aq) + OH–(aq)
NH4Cl(s) H2O NH4+(aq) + Cl–(aq)
NH (g)
NH4NO3(s) H2O NH4+(aq) + NO3–(aq)
HO
NaCl(s) 2 Na+(aq) + Cl–(aq)
Least Active
Least Active
LiBr(s) H2O Li+(aq) + Br–(aq)
Reference Tables for Physical Setting/Chemistry – 2011 Edition
5
**Activity Series is based on the hydrogen standard. H2 is not a metal.
379 © UNIT 10: OXIDATION & REDUCTION