of 1 mole of a monatomic gas is increased from 25°C to 300°C. 3.20 One mole of an ideal gas undergoes an isotherma expansion at 300 K from 1.00 atm to a final pressure while performing 200 J of expansion work. Calculate the final pressure of the gas if the external pressure s 0.20 atm. Heat Capacities 3.21 A 6.22-kg piece of copper metal is heated from 20.5° C to 324.3°C. Given that the specific heat of Cu is 0.385 J g1 °C-1, calculate the heat absorbed (in kJ) by the metal. 3.22 A 10.0-g sheet of gold with a temperature of 18.0°C is laid flat on a sheet of iron that weighs 20.0 g and has a temperature of 55.6°C. Given that the specific heats of Au and Fe are 0.129 J g-1 C-1 and 0.444 Jg-1 oc1, respectively, what is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. (Hint: The heat gained by the gold must be equal to the heat lost by the iron.) 3.23 It takes 330 joules of energy to raise the tempera- ture of 24.6 g of benzene from 21.0°C to 28.7°C at con stant pressure. What is the zene at constant pressure? 3.24 The molar heat of vaporization for water is 44.0 kJ mol-1 at 298 K and 40.79 kJ mol- qualitative explanation of th values. molar heat capacity of ben- 1 at 373 K. Give a e difference in these two 3.25 The constant-pressure molar heat capacit y of ni-

Chemistry & Chemical Reactivity
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Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
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3.22

of 1 mole of a monatomic gas is increased from 25°C to
300°C.
3.20 One mole of an ideal gas undergoes an isotherma
expansion at 300 K from 1.00 atm to a final pressure
while performing 200 J of expansion work. Calculate
the final pressure of the gas if the external pressure s
0.20 atm.
Heat Capacities
3.21 A 6.22-kg piece of copper metal is heated from
20.5° C to 324.3°C. Given that the specific heat of Cu is
0.385 J g1 °C-1, calculate the heat absorbed (in kJ) by
the metal.
3.22 A 10.0-g sheet of gold with a temperature of
18.0°C is laid flat on a sheet of iron that weighs 20.0 g
and has a temperature of 55.6°C. Given that the specific
heats of Au and Fe are 0.129 J g-1 C-1 and 0.444
Jg-1 oc1, respectively, what is the final temperature of
the combined metals? Assume that no heat is lost to the
surroundings. (Hint: The heat gained by the gold must
be equal to the heat lost by the iron.)
3.23 It takes 330 joules of energy to raise the tempera-
ture of 24.6 g of benzene from 21.0°C to 28.7°C at con
stant pressure. What is the
zene at constant pressure?
3.24 The molar heat of vaporization for water is 44.0
kJ mol-1 at 298 K and 40.79 kJ mol-
qualitative explanation of th
values.
molar heat capacity of ben-
1 at 373 K. Give a
e difference in these two
3.25 The constant-pressure molar heat capacit
y of ni-
Transcribed Image Text:of 1 mole of a monatomic gas is increased from 25°C to 300°C. 3.20 One mole of an ideal gas undergoes an isotherma expansion at 300 K from 1.00 atm to a final pressure while performing 200 J of expansion work. Calculate the final pressure of the gas if the external pressure s 0.20 atm. Heat Capacities 3.21 A 6.22-kg piece of copper metal is heated from 20.5° C to 324.3°C. Given that the specific heat of Cu is 0.385 J g1 °C-1, calculate the heat absorbed (in kJ) by the metal. 3.22 A 10.0-g sheet of gold with a temperature of 18.0°C is laid flat on a sheet of iron that weighs 20.0 g and has a temperature of 55.6°C. Given that the specific heats of Au and Fe are 0.129 J g-1 C-1 and 0.444 Jg-1 oc1, respectively, what is the final temperature of the combined metals? Assume that no heat is lost to the surroundings. (Hint: The heat gained by the gold must be equal to the heat lost by the iron.) 3.23 It takes 330 joules of energy to raise the tempera- ture of 24.6 g of benzene from 21.0°C to 28.7°C at con stant pressure. What is the zene at constant pressure? 3.24 The molar heat of vaporization for water is 44.0 kJ mol-1 at 298 K and 40.79 kJ mol- qualitative explanation of th values. molar heat capacity of ben- 1 at 373 K. Give a e difference in these two 3.25 The constant-pressure molar heat capacit y of ni-
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