Nelson Chemistry Chapter 11 Quiz
Click on the correct answer
1
The standard heat of formation for one mole of liquid water is
+4.19 J/g
o
C
+6.03 kJ/mol
+40.8 kJ/mol
-285.8 kJ/mol
2
Use the following information to answer this question.
Q
2
(g) ------> Q(g) + Q(g) delta H = +100 Kj/mol
X
2
(g) ------> X(g) + X(g) delta H = + 50 kJ/mol
Q(g) + X(g) -----> QX(g) delta H = -200 kJ/mol
If Q
2
(g) reacted with X
2
(g) to form QX(g), the statement that would best describe this reaction is that:
intramolecular bonding in sample X
2
(g) is stronger than in Q
2
(g)
intermolecular bonding in sample X
2
(g) is weaker than in Q
2
(g)
the reaction is endothermic
the reaction is exothermic
3
Use the following information to answer this question.
The molar heat of combustion for ethylene glycol, C
2
H
4
(OH)
2
(l), is -1181.2 kJ/mol when the products of combustion are gases.
The heat of formation of ethylene glycol is:
+590.6 kJ/mol
-331.2 kJ/mol
-500.7 kJ/mol
-1181.2 kJ/mol
4
The heat of formation of sodium chlorate [NaClO
3
(s)] is -53 kJ/mol. The balanced equation which expresses this information is
Na(s) + Cl
2
(g) + O
2
(g) -------> NaClO
2
(g) + 53 kJ
Na(s) +
1
/
2
Cl
2
(g) +
3
/
2
O
2
(g) -----> NaClO
3
(s) + 53 kJ
Na(s) +
1
/
2
Cl
2
(g) +
3
/
2
O
2
(g) + 53 kJ -------> NaClO
3
(s)
Na(s) + Cl
2
(g) + 3O
2
(g) ------> NaClO
3
(g) + 53 kJ
5
Use the following information to answer this question.
C(s) + 2H
2
(g) -----> CH
4
(g) delta H = -74.8 kJ
C(s) + 2Cl
2
(g) ------> CCl
4
(l) delta H = -106.4 kJ
1
/
2
H
2
(g) +
1
/
2
Cl
2
(g) -----> HCl(g) delta H = - 92.3 kJ
The heat of reaction for CH
4
(g) + 4Cl
2
(g) -----> CCl
4
(l) + 4HCl(g) is
-123.9 kJ
-216.2 kJ
-273.5 kJ
-400.8 kJ
6
Use the following information to answer this question.
6CO
2
(g) + 6H
2
O(l) + 2802.7 kJ ------> C
6
H
12
O
6
(s) + 6O
2
(g)
The amount of CO
2
(g) required to react so that 2.2 x 10
3
kJ are absorbed is:
7.6 mol
6.0 mol
4.7 mol
1.3 mol
7
A reaction has a positive delta H value. This means that
the reaction is exothermic
the reaction releases energy
during the reaction, the surroundings get colder
the heat content of the products is less than that of the reactants.
8
Which statement is correct?
H
f(products)
= H
f(reactants)
delta H = nH
f(products)
- nH
f(reactants)
delta H = nH
f(reactants)
- nH
f(products)
nH
f(products)
= delta H - nH
f(reactants)
9
Given the following thermochemical data:
1) C
2
H
2
(g) +
5
/
2
O
2
(g) -----> 2CO
2
(g) + H
2
O(l) delta-H = -1.30 x 10
3
kJ
2) C
2
H
6
(g) +
7
/
2
O
2
(g) -----> 2CO
2
(g) + 3H
2
O(l) delta-H = -1.56 x 10
3
kJ
3) H
2
(g) +
1
/
2
O
2
(g) -----> H
2
O(l) delta-H = -2.86 x 10
2
kJ
What is the delta-H for the reaction:
C
2
H
2
(g) + 2H
2
(g) -----> C
2
H
6
(g) delta-H = ?
-2.60 x 10
1
kJ
-3.12 x 10
2
kJ
-5.72 x 10
2
kJ
-5.46 x 10
3
kJ
10
The change that is predicted to release the largest quantity of energy is
C(s) + O
2
(g) -----> CO
2
(g)
2NO
2
(g) -----> N
2
O
4
(g)
14
6
C ----->
0
-1
e +
14
7
N
CO
2
(s) -----> CO
2
(g)