Ap Chemistry Chapter 16 Multiple Choice Quiz Review With Answers - Malea Mullins, University School Of Jackson Page 2
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144.
A 100-mL sample of water is placed in a coffee cup calorimeter. When 1.0 g of an ionic
solid is added, the temperature decreases from 21.5°C to 20.8°C as the solid dissolves.
For the dissolving of the solid
Note that the temperature of the solution decreased from 21.5°C to 20.8°C, so the process is
endothermic!!
ΔH > 0
a.
ΔH = + for endothermic reactions
ΔS
b.
< 0
univ
The solid dissovles so ΔS
must be positive.
univ
ΔS
c.
< 0
sys
The solid dissolves so it has access to a larger volume (more positions) so ΔS
sys
will increase.
ΔS
d.
> 0
surr
ΔS
is negative for endothermic reactions.
surr
e.
none of these
5.
Which of the following result(s) in an increase in the entropy of the system?
I.
See diagram to the right. (Closed on reactant side/ open on product
side) (more positions, so increases S)
(g) Br
II.
Br
(ℓ)
2
2
(gas to liquid, so decreases S)
1
NaBr (s) Na
+1
III.
(aq) + Br
(aq)
(solid dissolves, more positions, so increases S)
(298 K) O
IV.
O
(373 K)
2
2
(moving faster, greater disorder, so increases S)
(1 atm, 298 K) NH
V.
NH
(3 atm, 298 K)
3
3
(increase P, so decrease V, less positions, so decreases S)
a.
I
b.
II, V
c.
I, III, IV
d.
I, II, III, IV
e.
I, II, III, V
6.
A mixture of hydrogen and chlorine remains unreacted until it is exposed to ultraviolet
light from a burning magnesium strip. Then the following reaction occurs very rapidly:
(g) 2 HCl (g)
H
(g) + Cl
2
2
ΔG = 45.54 kJ
(spontaneous because negative)
ΔH = 44.12 kJ
(exothermic because negative)
ΔS = 4.76 J/K
Both ΔH and ΔS are negative, so the reaction is
spontaneous at low temperatures.
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