ANSWER on SEPARATE SHEET OF PAPER
ANSWER on SEPARATE SHEET OF PAPER
Thermodynamics Worksheet
Thermodynamics Worksheet
1. ΔHfusion = 6.01kj/mol, ΔHvaporization = 41.0 kJ/mol, and SH = 4.18J/g*C
a. How much heat must be added to melt 90g of ice if its
temperature is -4 C?
b. How much heat must be added to raise the resulting liquid to its
boiling point of 100C?
c. How much heat must be added to convert all the liquid into
vapor?
d. What is the total energy added in kJ?
1. ΔHfusion = 6.01kj/mol, ΔHvaporization = 41.0 kJ/mol, and SH = 4.18J/g*C
a. How much heat must be added to melt 90g of ice if its
temperature is -4 C?
b. How much heat must be added to raise the resulting liquid to its
boiling point of 100C?
c. How much heat must be added to convert all the liquid into
vapor?
d. What is the total energy added in kJ?
2. Southern California is running short of fresh drinking water. A student
suggested that large icebergs be towed from Antarctica and be melted
for drinking water. The melting of ice to water has a ΔHvaporization of
6.01 kJ
H 2O(s)  H 2O(l)
ΔH = 6.01kJ
2. Southern California is running short of fresh drinking water. A student
suggested that large icebergs be towed from Antarctica and be melted
for drinking water. The melting of ice to water has a ΔHvaporization of
6.01 kJ
H 2O(s)  H 2O(l)
ΔH = 6.01kJ
How much energy would be required to melt an iceberg that has a mass of
1000kg?
How much energy would be required to melt an iceberg that has a mass of
1000kg?
3. How much ice at -15.0 C is needed to freeze 1.00 kg of water at 25 C?
ΔHfusion = 6.01kj/mol, ΔHvaporization = 41.0 kJ/mol, and
SH of ice = 2.03 J/g*C
3. How much ice at -15.0 C is needed to freeze 1.00 kg of water at 25 C?
ΔHfusion = 6.01kj/mol, ΔHvaporization = 41.0 kJ/mol, and
SH of ice = 2.03 J/g*C
4. How much heat is released when 200. g of steam at 115 C cools to
room temp? ΔHfusion = 6.01kj/mol, ΔHvaporization = 41.0 kJ/mol, and
SH of water = 4.18 J/g*C SH of steam = 2.01 J/g*C
4. How much heat is released when 200. g of steam at 115 C cools to
room temp? ΔHfusion = 6.01kj/mol, ΔHvaporization = 41.0 kJ/mol, and
SH of water = 4.18 J/g*C SH of steam = 2.01 J/g*C
5. What is the specific heat capacity of mercury if it requires 167.0 J to
change the temperature of 15.0 g mercury from 25.00C to 33.00C?
5. What is the specific heat capacity of mercury if it requires 167.0 J to
change the temperature of 15.0 g mercury from 25.00C to 33.00C?
6.
2Al(s) + Fe2O3(s)  2Fe(s) + Al2O3
ΔH = -851.5kJ
If 17.3 g of Al reacted with excess Fe2O3(s), how much heat is released?
6.
2Al(s) + Fe2O3(s)  2Fe(s) + Al2O3
ΔH = -851.5kJ
If 17.3 g of Al reacted with excess Fe2O3(s), how much heat is released?
7. The ΔH value for the reaction ½ O2(g) + Hg(l)  HgO(s) is –90.8 kJ. How
much heat is released when 32.5 g Hg is reacted with oxygen?
7. The ΔH value for the reaction ½ O2(g) + Hg(l)  HgO(s) is –90.8 kJ. How
much heat is released when 32.5 g Hg is reacted with oxygen?
8. The total volume of hydrogen gas needed to fill the Hindenburg was
2.00 x 108 L at 1.00 atm and 25.0C. How much energy was evolved
when it burned?
H2(g) + ½ O2(g)  H2O(l), ΔH = –286 kJ
8. The total volume of hydrogen gas needed to fill the Hindenburg was
2.00 x 108 L at 1.00 atm and 25.0C. How much energy was evolved
when it burned?
H2(g) + ½ O2(g)  H2O(l), ΔH = –286 kJ
9. Calculate ΔH for C2H4(g) + H2(g)  C2H6(g)
Given: C2H2(g) + H2(g)  C2H4(g)
C2H2(g) + 2H2(g)  C2H6(g)
9. Calculate ΔH for C2H4(g) + H2(g)  C2H6(g)
Given: C2H2(g) + H2(g)  C2H4(g)
C2H2(g) + 2H2(g)  C2H6(g)
ΔH = -175.7kJ
ΔH = -312.0kJ
ΔH = -175.7kJ
ΔH = -312.0kJ
10. Calculate ΔH for 2N2(g) + 6H2O(g)  3O2(g) + 4NH3(g)
Given: NH3(g)  ½ N2(g) + 3/2 H2(g) ΔH = 46kJ
2H2(g) + O2(g) 2H2O(g)
ΔH = - 484kJ
10. Calculate ΔH for 2N2(g) + 6H2O(g)  3O2(g) + 4NH3(g)
Given: NH3(g)  ½ N2(g) + 3/2 H2(g) ΔH = 46kJ
2H2(g) + O2(g) 2H2O(g)
ΔH = - 484kJ
11. How are heat capacity and specific heat different from one another? If
there was a 10 lb block of iron and a 1 lb block of iron, would both
objects have the same heat capacity? If not, why? Would the objects
have the same specific heat? Why?
11. How are heat capacity and specific heat different from one another? If
there was a 10 lb block of iron and a 1 lb block of iron, would both
objects have the same heat capacity? If not, why? Would the objects
have the same specific heat? Why?
12. When a substance, such as water is changing phases, what happens to
the temperature of that substance? In other words, as solid ice is
melting over a hot flame, what is happening to the temperature and
why?
12. When a substance, such as water is changing phases, what happens to
the temperature of that substance? In other words, as solid ice is
melting over a hot flame, what is happening to the temperature and
why?