MSE227
Homework Answers
Chapters 15 & 16
Chapter 15
15.1
You should have used the rule of mixtures approach to generate the curves below:
15.4
cl* = 1640 MPa
Ecl = 60.3 GPa
15.7
(a)
(b)
(c)
(d)
15.11 (a)
Ff = 44.7 Fm
Fm – 1168 N
f = 242 MPa
m = 4.4 MPa
m = 1.84 x 10-3
Specific Strength:
Glass/Fiber: 486 MPa
Carbon Fiber: 775 MPa
Aramid Fiber (Kevlar): 986 MPa
Cold rolled 7-7PH: 180 MPa
1040 plain carbon : 75 MPa
7075 T6 Al: 204 MPa
C2600 brass: 62 MPa
AZ31B Mg: 148 MPa
Ti-5Al-2.5Sn: 176 MPa
(b)
Specific Modulus:
glass-fiber reinforced epoxy: 21.4 GPa
carbon-fiber reinforced epoxy: 90.6 GPa
aramid-fiber reinforced epoxy: 54.3 GPa
cold rolled 17-7PH stainless steel: 26.7 GPa
1040 plain-carbon steel: 26.4 GPa
7075-T6 Al: 25.4 GPa
C26000 brass: 12.9 GPa
AZ31B Mg: 25.4 GPa
Ti-5Al-2.5Sn: 24.6 GPa
15D2
Such a composite is possible if 0.353 < Vf < 0.391.
Chapter 16
16.1 (a) The possible oxidation and reduction half-reactions for magnesium in various
solutions are as follows:.
(i) In HCl, possible reactions are
Mg  Mg 2+ + 2e- (oxidation)

2H+ + 2e-  H2 (reduction)
(ii) In an HCl solution containing dissolved oxygen, possible reactions are

Mg  Mg 2+ + 2e- (oxidation)

4H+ + O2 + 4e-  2H2O (reduction)
(iii) In an HCl solution containing dissolved oxygen and Fe2+ ions, possible reactions
are

Mg  Mg 2+ + 2e- (oxidation)


4H+ + O2 + 4e-  2H2O (reduction)
Fe 2+ + 2e-  Fe (reduction)
(b) The magnesium would probably oxidize most rapidly in the HCl solution containing

dissolved oxygen and Fe2+ ions because there are two reduction reactions that will consume
electrons from the oxidation of magnesium.
16.2
(a)
(b)
V = -0.011 V
Since the V is negative, the spontaneous cell direction is just the reverse of that
in (a), or
Sn 2+ + Pb  Sn + Pb 2+
16.12 For each of the forms of corrosion, the conditions under which it occurs, and measures
that may be taken to prevent or control it are outlined in Section 16.7.

16.13 For a small anode-to-cathode area ratio, the corrosion rate will be higher than for a large
ratio. The reason for this is that for some given current flow associated with the
corrosion reaction, for a small area ratio the current density at the anode will be greater
than for a large ratio. The corrosion rate is proportional to the current density (i)
according to Equation 16.24.
16.D1 (a) Laboratory bottles to contain relatively dilute solutions of nitric acid. Probably the
best material for this application would be polytetrafluoroethylene (PTFE). The reasons
for this are: (1) it is flexible and will not easily break if dropped; and (2) PTFE is
resistant to this type of acid, as noted in Table 16.4.
(b) Barrels to contain benzene. Poly(ethylene terephthalate) (PET) would be suited for
this application, since it is resistant to degradation by benzene (C6H6) (Table 16.4), and
is less expensive than the other three materials listed as satisfactory (S) in Table 16.4 (see
Appendix C for cost data).
(c) Pipe to transport hot alkaline (basic) solutions. The best material for this application
would probably be a nickel alloy (Section 13.3). Polymeric materials listed in Table 16.4
would not be suitable inasmuch as the solutions are hot.
(d) Underground tanks to store large quantities of high-purity water. The outside of the
tanks should probably be some type of low-carbon steel that is cathodically protected
(Sections 16.8 and 16.9). Inside the steel shell should be coated with an inert polymeric
material; polytetrafluoroethylene or some other fluorocarbon would probably be the
material of choice (Table 16.4).
(e) Architectural trim for high-rise buildings. The most likely candidate for this
application would probably be an aluminum alloy. Aluminum and its alloys are
relatively corrosion resistant in normal atmospheres (Section 16.8), retain their lustrous
appearance, and are relatively inexpensive (Appendix C).