Chapter 17 Practice Quiz 2014
Moore/Tallman
Name:___________________
Period_______
1. A thermometer is in a beaker of water. Which statement
best explains why the thermometer reading initially
increases when LiBr(s) is dissolved in the water?
A) The entropy of the LiBr(aq) is greater than the
entropy of the water.
B) The entropy of the LiBr(aq) is less than the entropy
of the water.
C) The dissolving of the LiBr(s) in water is an
endothermic process.
D) The dissolving of the LiBr(s) in water is an
exothermic process.
2. In a chemical reaction, the difference between the
potential energy of the products and the potential energy
of the reactants is equal to the
A) activation energy
C) heat of reaction
B) kinetic energy
D) rate of reaction
3. Given: C 2H6(g) ® C2H2(g) + 2 H 2(g)
–1
DH° = +1340 kJ•mol
An alternate way to write this equation is:
A)
B)
C)
D)
E)
C2H6(g) + 1340 kJ ® C2H2(g) + 2 H 2(g)
C2H2(g) + 2 H 2(g) + 1340 kJ ® C2H6(g)
C2H6(g) ® C2H2(g) + 2 H 2(g) + 1340 kJ
C2H2(g) + 2 H 2(g) ® C2H6(g) + 1340 kJ
C2H6(g) – 1340 kJ ® C2H2(g) + 2 H 2(g)
4. Use the values of the standard heat of formation in the
table to calculate the heat of reaction, DH°, for the
reaction
A) –7640 kJ
C) +2,240 kJ
E) +5,290 kJ
B) –265 kJ
D) –13,400 kJ
5. Given the equations:
12 O2(g)+ H 2(g) ® H2O(g)+ 243 kJ
12 O2(g) + 2H(g) ® H2O(g) + 661 kJ
How much energy is needed to dissociate 1.00 mole of
H2 according to the equation below?
H2(g) ® 2H(g)
A) 243 kJ
C) 661. kJ
E) 1320 kJ
B) 418 kJ
D) 904. kJ
6. Consider the equations:
C(s) + O 2(g) ® CO 2(g) DH= –394kJ•mol –1
–1
CO(g) + O2(g) ® CO 2(g) DH= –283kJ•mol
this information, calculate DH of the equation
C(s) + O2(g) ® CO(g)
A) –111 kJ•mol–1
C) –394 kJ•mol–1
E) +283 kJ•mol–1
7. I. A negative
reaction.
From
B) –283 kJ•mol–1
D) –577 kJ•mol–1
H ( – H) indicates an exothermic
BECAUSE
II. with a negative
than the reactants.
A)
B)
C)
D)
H, the products have more energy
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
8. I. Heat is released with an endothermic reaction
BECAUSE
II. energy is released when bonds are formed.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
9. I. A positive DH tells you that the reaction is exothermic
BECAUSE
II. with a positive DH, the products have more energy
than the reactants.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
E) I and II are BOTH TRUE and II IS a correct
explanation of I
10. Base your answer to the following question on
the information below.
Ammonium chloride is dissolved in water to form a 0.10 M NH4Cl(aq) solution. This dissolving process
is represented by the equation below.
State evidence that indicates the dissolving of ammonium chloride is an endothermic process.
11. To break a chemical bond, energy must be
A) absorbed
C) produced
B) destroyed
D) released
12. What occurs in order to break the bond in a Cl2
molecule?
A)
B)
C)
D)
Energy is absorbed.
Energy is released.
The molecule creates energy.
The molecule destroys energy.
13. Given the balanced equation representing a reaction:
Cl 2
Cl + Cl
What occurs during this reaction?
A)
B)
C)
D)
A bond is broken as energy is absorbed.
A bond is broken as energy is released.
A bond is formed as energy is absorbed.
A bond is formed as energy is released.
14. For a chemical reaction, the heat of reaction is equal to
the
A) potential energy of the reactants, only
B) potential energy of the products, only
C) potential energy of the products plus the potential
energy of the reactants
D) potential energy of the products minus the
potential energy of the reactants
15. Given the balanced equation:
4Fe(s) + 3O 2(g)
2Fe2O3(s) + 1640 kJ
Which phrase best describes this reaction?
A)
B)
C)
D)
endothermic with H = +1640 kJ
endothermic with H = –1640 kJ
exothermic with H = +1640 kJ
exothermic with H = –1640 kJ
16. Which statement correctly describes an endothermic
chemical reaction?
A) The products have higher potential energy than the
reactants, and the H is negative.
B) The products have higher potential energy than the
reactants, and the H is positive.
C) The products have lower potential energy than the
reactants, and the H is negative.
D) The products have lower potential energy than the
reactants, and the H is positive.
A + B ® C + heat,
the potential energy of the products, compared to the
potential energy of the reactants, is
less and the reaction is exothermic
less and the reaction is endothermic
greater and the reaction is exothermic
greater and the reaction is endothermic
18. Given the reaction:
What is the heat of formation of nitrogen (II) oxide in
kJ/mole?
A)
C)
A) -16.69 kJ
C) -445.1 kJ
B) -667.7 kJ
20. When 25.7 grams of NaI dissolves in 80.0 grams of
water in a calorimeter, the temperature rises from 20.5
°C to 24.4 °C. Calculate H for the process.
A) -10.1kJ/mole
C) 1724.8 kJ/mole
B) -7.63 kJ/mole
D) -2.45 kJ/mole
21. 1. Calculate the amount of heat given off when 12.5g of
ethanol burns.
C2H5OH +3O2
2CO 2 +3H2O H = -1368 kJ/mol
22. 1. What is the standard heat of formation ( H) for the
following?
4NH 3 + 5O2
4NO + 6H2O
Hf NH 3 = -46.19kJ/mol Hf NO = 90.37kJ/mol Hf
H2O = -241.8kJ/mol
23. From the following enthalpy changes,
C2H6O(l) + 3O 2(g)
2CO 2(g) + 3H 2O(l) H =
-685.5 kJ
C2H4O(l) + 5/2O2(g)
2CO 2(g) + 2H 2O(l) H =
-583.5 kJ
Calculate the value of H for the reaction: 2C 2H4O(l)
+ 2H2O(l)
2C2H6O(l) + O 2(g)
24. From the following enthalpy changes,
S (s) + 3/ 2 O2 (g)
SO 3 (g) H° = -395.2 kJ
2 SO 2 (g) + O 2 (g) 2 SO 3 (g) H° = -198.2 kJ
17. For the reaction
A)
B)
C)
D)
19. How much heat is released when 1.5 grams of NaOH is
dissolved in water? Hsol=-445.1 kJ/mole
B)
D)
Calculate the value of
(g)
SO 2 (g)
H for the reaction: S (s) + O 2