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Test 2 - Review - PE Diagrams , Table I
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1) Which one of the following statements describes characteristics of an endothermic reaction?
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A) The sign of ΔH is positive, and the products have less potential energy than the reactants.
B) The sign of ΔH is negative, and the products have less potential energy than the reactants.
C) The sign of ΔH is negative, and the products have more potential energy than the reactants.
D) The sign of ΔH is positive, and the products have more potential energy than the reactants.
2) A student dissolved a salt in water and noted that the temperature of the water decreased during the dissolving process. A logical conclusion based on this observation is that the salt
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A) oxidized in water
B) dissolved exothermically D) ionized in water
C) dissolved endothermically
D) ionized in water
3. Given the equation: I + I → I2 + 146 kJ. This equation shows that the formation of an iodine molecule is an
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A) endothermic process in which energy is released
B) endothermic process in which energy is absorbed
C) exothermic process in which energy is absorbed
D) exothermic process in which energy is released
4. Consider the reaction below. Which one of the following phrases best describes this reaction?
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A) exothermic, absorbing energy
B) endothermic, releasing energy
C) exothermic, releasing energy
D) endothermic, absorbing energy
5) Energy is released when the atoms of two elements bond to form a compound. Compared to the total potential energy of the atoms before bonding, the total potential energy of the atoms after bonding is
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A) lower and the compound formed is unstable
B) lower and the compound formed is stable
C) higher and the compound formed is stable
D) higher and the compound formed is unstable
6. In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is the
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A) heat of reaction
B) free energy
C) activation energy
D) heat of fusion
7. What change does the ΔH of a chemical reaction represent?
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A) activation energy
B) heat of reaction
C) entropy D) free energy
D) free energy
8. For which compound is the process of dissolving in water exothermic?
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A) NaOH
B) NH4Cl
C) NaCl
D) NH4NO
9. A thermometer is in a beaker of water. Which one of the following statements best explains why the thermometer reading initially increases when LiBr(s) is dissolved in the water?
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A) The entropy of the LiBr(aq) is greater than the entropy of the water.
B) The dissolving of the LiBr(s) in water is an exothermic process.
C) The entropy of the LiBr(aq) is less than the entropy of the water.
D) The dissolving of the LiBr(s) in water is an endothermic process.
10. Given the balanced equation representing a reaction below, which one of the following statements is true about this reaction?
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A) It is exothermic and ΔH equals −91.8 kJ.
B) It is exothermic and ΔH equals +91.8 kJ.
C) It is endothermic and ΔH equals +91.8 kJ.
D) It is endothermic and ΔH equals −91.8 kJ.
11. Which equation represents an exothermic reaction at 298 K?
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A
B
C
D
12. Which compound is formed from its elements by an exothermic reaction at 298 K and 101.3 kPa?
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A
B
C
D
13. At 101.3 kPa and 298 K, what is the total amount of heat released when one mole of aluminum oxide,Al O (s), is formed from its elements?
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A) 393.5 kJ
B) 3,351 kJ
C) 1,676 kJ
D) 837.8 kJ
14. Given the balanced equation representing a reaction below, what is the net amount of energy released when one mole of H2O(ℓ) is produced?
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A) 241.8 kJ
B) 483.6 kJ
C) 571.6 kJ
D) 285.8 kJ
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