Chemistry Reference
In-Depth Information
14.43 Calculate the final temperature after 10.7 g of aluminum
at is placed in 117 g of water at
14.44 Calculate the final temperature after 2.47 g of zinc at
is placed in 29.4 g of water at
14.45 Calculate the final temperature after 29.4 g of cobalt at
is placed in 94.3 g of water at
14.46 How much energy is required to raise the temperature of
10.0 g of chromium from to
14.47 Calculate the final temperature after 14.9 g of an alloy of
metals
14.57
Calculate the enthalpy of formation of
CH
2
O
from the
72.3°C
14.6°C.
following data:
H
(kJ)
60.1°C
16.4°C.
CH
2
O
O
2
£ CO
2
H
2
O
561
1
2
O
2
H
2
O £ H
2
286
15.9°C
61.4°C.
CO
2
£ C
O
2
393
14.58 Calculate for the reaction of 14.9 g of CuO accord-
ing to the equation
¢
H
41.3°C
104.0°C?
(
c
0.650 J/g
#
°C)
3 CuO(s)
CH
4
(g) £ CO(g)
2 H
2
O(
/
)
3 Cu(s)
at
81.6°C
is placed in 88.8 g
of water at
14.48
A certain reaction emits 3.95 kJ of heat. What tempera-
ture change will 250.0 g of water at
15.5°C.
14.59
Calculate the enthalpy of combustion at
25°C
of 125 g
of CO.
16.0°C
undergo if
14.60
Given the following information:
the heat from the reaction is added to it?
14.49
Calculate the heat required to change 27.7 g of ice at
to liquid water at
14.50 Calculate the heat required to change 255 g of liquid wa-
ter at to water vapor at
14.51
Calculate the final temperature after 17.0 g of water at
is mixed with (a) 17.0 g water at
X £ Q
Z
¢
H
°
27.0 kJ
R
15.9°C
25.0°C.
Q
Z £ T
¢
H
°
43.0 kJ
¢
calculate
H
° for each of the following reactions:
88.5°C
125.0°C.
X £ T
(a)
(b)
(c)
R
Q
Z £ R
X
20.0°C
50.0°C
(b) 34.0 g
of water at
50.0°C.
2 Q
2 Z £ 2 R
2 X
14.4 Enthalpy Changes in Chemical Reactions
14.61
Calculate the enthalpy change for the following reaction
of sucrose and water to give glucose and fructose, from
their enthalpies of
combustion,
given below each sub-
stance in the following equation:
14.52
Write an equation corresponding to the
¢
H
for the
(a) Sublimation of ice
(b) Formation of carbon monoxide
(c) Formation of carbon dioxide
(d) Combustion of carbon
(e) Which two of the preceding are the same?
14.53 Write an equation to which each of the following corre-
sponds:
(a) (b)
(c) (d)
(e) (f)
14.54
Write a balanced chemical equation corresponding to the
reaction with enthalpy change given as (a)
and (b)
14.55 Which of the following processes represents the reaction
corresponding to the enthalpy of formation of AgCl?
Explain.
(a)
(b)
(c)
(d)
14.56
(a) Write a balanced chemical equation for the complete
combustion of formaldehyde, (b) Its enthalpy
of combustion is Calculate its enthalpy
of formation. (c) Calculate the enthalpy change when
68.3 g of the compound is burned.
C
12
H
22
O
11
(s)
H
2
O(
/
) £ C
6
H
12
O
6
(s)
C
6
H
12
O
6
(s)
Sucrose
Glucose
Fructose
5648 kJ/mol
2816 kJ/mol
2824 kJ/mol
¢
H
X
Q £ Z
14.62 The value of
for the reaction
is 13.3 kJ.
¢
H
What is the value of
for each of the following
reactions?
(a)
2 X
2 Q £ 2 Z
Y
(b)
Z £ Q
¢
H
sublimation
(CO
2
)
¢
H
f
(CO)
14.63
Which of the following equations represents the enthalpy
of combustion of
¢
H
combustion
(CO)
¢
H
fusion
(H
2
O)
C
6
H
14
O?
Explain why.
¢
H
f
(HCl)
¢
H
combustion
(CH
4
)
C
6
H
14
O(
/
)
6 O
2
(g) £ 6 CO(g)
7 H
2
O(
/
)
C
6
H
14
O(
/
)
9 O
2
(g) £ 6 CO
2
(g)
7 H
2
O(
/
)
¢
H
f
(C
8
H
18
)
¢
H
combustion
(C
8
H
18
).
14.64 Which of the following equations
(i)
(ii)
(iii)
(iv)
(v)
have enthalpy changes equal to
(a)
(b)
(c)
(d)
¢
H
f
(CO)
O
2
(g) £ CO
2
(g)
C
(graphite)
1
2
O
2
(g) £ CO
2
(g)
CO(g)
1
2
O
2
(g) £ CO(g)
C
(graphite)
1
2
Cl
2
(g)
AgCl(s) £ Ag(s)
1
2
O
2
(g) £ CO(g)
C
(diamond)
1
2
Cl
2
(g) £ AgCl(s)
Ag(s)
O
2
(g) £ CO
2
(g)
C
(diamond)
Ag
(aq)
Cl
(aq) £ AgCl(s)
Ag(s)
AuCl(s) £ Au(s)
AgCl(s)
¢
H
f
(CO
2
)
CH
2
O.
¢
H
combustion
(C)
561 kJ/mol.
¢
H
combustion
(CO)
