Question

Which will have the smallest temperature change for a given addition of energy?

Select one:

a. 10.00 g gold (*c* = 25.4 J/mol • °C)

b. 10.00 g water (*c* = 75.3 J/mol • °C)

c. 5.00 g gold (*c* = 25.4 J/mol • °C)

d. 5.00 g water (*c* = 75.3 J/mol • °C)

Answer #1

We know that heat energy , Q = mcdt

Where

m = mass

c = specific heat capacity

dt = change in temperature

For the given compounds product of m & c are as follows:

a. 10.00 g gold (c = 25.4 J/mol • °C= 25.4J/(197 g
^{o}C) = 0.13 J/g^{o}C) ----> 10.00x0.13 =
**1.3** J/^{o}C

b. 10.00 g water (*c* = 75.3 J/mol • °C= 75.3 J/(18 g
^{o}C) = 4.18 J/g^{o}C) ----> 10.00x4.18 =
**41.8** J/^{o}C

c. 5.00 g gold (*c* = 25.4 J/mol • °C= 25.4J/(197 g
^{o}C) = 0.13 J/g^{o}C) ----> 5.00x0.13 =
**0.65** J/^{o}C

d. 5.00 g water (*c* = 75.3 J/mol • °C= 75.3 J/(18 g
^{o}C) = 4.18 J/g^{o}C) ----> 5.00x4.18 =
**20.9** J/^{o}C

For a given addition of energy smallest temperature change will
occur for (b) 10.00 g water (*c* = 75.3 J/mol.°C) since it
has highest value **41.8** J/^{o}C

Therefore option (b) is correct.

Based on the thermodynamic properties provided for water,
determine the energy change when the temperature of 1.15 kg of
water decreased from 113 °C to 40.5 °C.
Property
Value
Units
Melting point
0
°C
Boiling point
100.0
°C
ΔHfus
6.01
kJ/mol
ΔHvap
40.67
kJ/mol
cp (s)
37.1
J/mol · °C
cp (l)
75.3
J/mol · °C
cp (g)
33.6
J/mol · °C

Based on the thermodynamic properties provided for water,
determine the energy change when the temperature of 0.550 kg of
water decreased from 111 °C to 30.5 °C.
Property
Value
Units
Melting point
0
°C
Boiling point
100.0
°C
ΔHfus
6.01
kJ/mol
ΔHvap
40.67
kJ/mol
cp (s)
37.1
J/mol ·°C
cp (l)
75.3
J/mol ·°C
cp (g)
33.6
J/mol ·°C

Based on the thermodynamic properties provided for water,
determine the energy change when the temperature of 0.350 kg of
water decreased from 123 °C to 30.0 °C.
Property
Value
Units
Melting point
0
°C
Boiling point
100.0
°C
ΔHfus
6.01
kJ/mol
ΔHvap
40.67
kJ/mol
cp (s)
37.1
J/mol ·°C
cp (l)
75.3
J/mol ·°C
cp (g)
33.6
J/mol ·°C

Based on the thermodynamic properties provided for water,
determine the energy change when the temperature of 1.45 kg of
water decreased from 117 °C to 23.5 °C.
Property
Value
Units
Melting point
0
°C
Boiling point
100.0
°C
ΔHfus
6.01
kJ/mol
ΔHvap
40.67
kJ/mol
cp
(s)
37.1
J/mol · °C
cp
(l)
75.3
J/mol · °C
cp
(g)
33.6
J/mol · °C

Based on the thermodynamic properties provided for water,
determine the energy change when the temperature of 1.25 kg of
water decreased from 125 °C to 24.5 °C.
Melting point: 0 degrees C
Boiling Point: 100 degrees C
Delta H(fus): 6.01 kJ/mol
Delta H(vap): 40.67 kJ/mol
cp(s): 37.1 J/mol x degrees C
cp(l): 75.3 J/mol x degrees C
cp(g): 33.6 J/mol x degrees C

A)
Given the following heat capacities of materials, which one,
assuming equal mass and temperature changes, would be best able to
store the smallest amount of thermal energy?
Group of answer choices
100 J/(kg °C)
0.1 J/(kg °C)
1 J/(kg °C)
1000 J/(kg °C)
B)
Given the following heat capacities of materials, which one,
assuming equal mass and temperature changes, would be best able to
store the largest amount of thermal energy?
k is the metric prefix for 1000
Group...

Adding nitric acid to water is quite exothermic. Calculate the
temperature change of 100 mL of water (d = 1.00g/mL) at
19.8°C [cp = 75.3 J/(mol·°C)] after adding 10.0 mL of
concentrated HNO3(14.5M , ΔH°soln = –33.3 kJ/mol). Assume
the concentrated HNO3 has a density equal to that of water.

How does the temperature change in the water correlate
to the change in the reaction????????????????
Trial 1
Trial 2
mass of baking powder (Na2cO3) added
3g
3g
mass of vinegar added
43.3 g
43.3 g
Final
temperature, tf
19.3°C
19.3°C
Initial temperature, ti
21.2°C
21.2C
Change in temperature, ∆t
1.9°C
1.9°C
q (water) = mwCwTw
368.06648 J
368.06648 J
q(reaction)
- 368.06648 J
- 368.06648 J
moles of Na2CO3
0.02830 mol
0.02830 mol
ΔH (kJ/mol)
13.006 kj/mol
13.006 kj/mol
S

What is the total energy (in Joules) required to raise
the temperature of 630 g of water from 20degC to 110degC? Please
draw this change on a heating curve making sure to label the
starting temperature, ending temperature and phase change.
ΔHfus = +6.01kJ/mol
ΔHvap = +40.7 kJ/mol
csteam = 2.02 J/g degC
Cice = 2.01 J/g degC

1) If the same quantity of energy is added to 10.00 g pieces of
gold, magnesium and platinum, all originally at 25°C, which metal
will have the highest final temperature? What is that
temperature?
CAu = 25.41 J/mol°C, CMg = 24.79 J/mol°C,
CPt = 25.95 J/mol°C
2) Acetylene (C2H2) and benzene
(C6H6) have the same empirical formula and
benzene can be synthesized from acetylene:
3C2H2(g)------------->
C6H6(l)
Find ∆Hreaction for the synthesis of benzene using
the ∆Hf° values below.
C6H6 –3267.4...

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