1. Energy that an object possesses by virtue of its position relative to other objects.
a. kinetic energy
b. potential energy
c. heat energy
d. light energy
2. Energy of an object due to the motion of an object.
a. chemical energy
b. heat energy
c. kinetic energy
d. potential energy
3. The SI unit of energy is
a. calorie
b. joule
c. atm
d. kg. m
4. It is an energy that is transferred from a hotter object to a colder one.
a. chemical energy
b. heat energy
c. internal energy
d. kinetic energy
5. It is the sum of all kinetic energy and potential energy of its component parts.
a. chemical energy
b. heat energy
c. internal energy
d. kinetic energy
6. Is a process in which the system absorbs heat from the surroundings.
a. exothermic
b. endothermic
c. spontaneous
d. nonspontaneous
7. Is a process in which the system releases heat to the surrounding.
a. exothermic
b. endothermic
c. spontaneous
d. nonspontaneous
8. An instrument used to measure the temperature change accompanying a process.
a. calorimeter
b. thermometer
c. speedometer
d. altimeter
9. Is a law that states that if a reaction is carried out in a series of steps, ∆H for the reaction will be equal to the sum of the enthalpy changes for the steps.
a. First Law of Thermodynamics
b. Second Law of Thermodynamics
c. Hess Law
d. Third Law of Thermodynamics
10. Is a law which states that energy is conserved during any process. It is just transformed from one form of energy to another form of energy.
a. First Law of Thermodynamics
b. Second Law of Thermodynamics
c. Hess Law
d. Third Law of Thermodynamics
11. Which metal requires the most energy to raise 1.00 g of it by 1.00oC?
a. aluminum
b. silver
c. iron
d. gold
12. Which process is exothermic?
a. the boiling of liquid nitrogen
b. the freezing of water
c. the sublimation of dry ice
d. the vaporization of water
13. Which statement correctly describes the energy changes that take place when a solid changes to a liquid at constant temperature.
a. The potential energy increases, and the kinetic energy remains constant.
b. The potential energy remains constant, and the kinetic energy increases.
c. The potential energy decreases, and the kinetic energy decreases.
d. The potential energy increases, and the kinetic energy decreases.
14. Why does warm water have a more rapid rate of evaporation than cold water?
a. It has a higher viscosity.
b. Its molecules have a higher average kinetic energy.
c. Its molecules have more attraction for one another.
d. More of its molecules have nearly the same kinetic energy.
15. What does it mean if the ∆H value for a chemical reaction is positive?
a. kinetic energy is increasing in the system
b. potential energy is decreasing in the system
c. products have less potential energy than reactants
d. reactants have less potential energy than products
16. What is 4.18 J?
a. The heat required to raise the temperature of one gram of water by one Celsius degree.
b. The heat required to raise the temperature of one mole of water by one Celsius degree.
c. The heat required to raise the temperature of one gram of substance by one Celsius degree.
d. The heat required to raise the temperature of one mole of substance by one Celsius degree.
17. What is a positive molar heat of formation?
a. The heat absorbed when one mole of compound is formed from its elements.
b. The heat released when one mole of compound is formed from its elements.
c. The heat absorbed when one mole of elements is formed from the compound.
d. The heat released when one mole of the elements is formed from the compound.
18. What change is probably happening when energy is added to a substance, but the substance's temperature does not rise?
a. gas to liquid
b. gas to solid
c. liquid to gas
d. liquid to solid
19. What occurs when solid A (50oC) is placed in contact with solid B (80oC?
a. Heat energy flows from A to B as the average kinetic energy of particles in A decreases.
b. Heat energy flows from A to B as the average kinetic energy of in A increases.
c. Heat energy flows from B to A as the average kinetic energy of B decreases.
d. Heat energy flows from B to A as the average kinetic energy of B increases.
20. What happens to the water in a calorimeter when an exothermic reaction occur in it?
a. It absorbs heat, and a drop in temperature is observed.
b. It absorbs heat, and a rise in temperature is observed.
c. It releases heat, and a drop in temperature is observed.
d. It releases heat, and a rise in temperature is observed.
21. Which is true for an exothermic reaction?
a. The ∆H is positive.
b. The products have less potential energy than the reactants.
c. The reactants have more kinetic energy than the products.
d. The reactants are below the products in the potential energy diagram.
22. Which statement is true?
a. An endothermic reaction is characterized by a negative value of ∆H.
b. An exothermic reaction transfer heat to the surroundings.
c. Heat is evolved when an endothermic reaction occurs.
d. The reaction vessels cools when an exothermic reaction occurs.
23. If the molar heat of fusion of sodium is 2.63 kJ/mol, how much energy is needed to melt 180.0 g of solid sodium at its melting point?
a, 2.63 kJ
b. 2.93 kJ
c. 20.6 kJ
d. 473 kJ
24. If the heat of fusion of a substance is 20 kJ/mol, how much heat is released when 1.0 mol of liquid at the melting point freezes?
a. 10 kJ
b. 20 kJ
c. 40 kJ
d. 80 kJ
25. Living plants produce glucose in the process of photosynthesis according to this equation:
6CO2(g) + 6H2O(l) + energy → C6H12O6(s) + 6O2(g)
Is this reaction endothermic or exothermic, and is the value of ∆Ho positive or negative?
a. endothermic, positive
b. endothermic, negative
c. exothermic, positive
d. exothermic, negative
26. In order to produce 972 kJ of heat, how many grams of H2 must burn?
a. endothermic, positive
b. endothermic, negative
c. exothermic, positive
d. exothermic, negative
26. In order to produce 972 kJ of heat, how many grams of H2 must burn?
H2(g) + 1/2 O2(g) → H2O(g) + 243 kJ
a. 0,250 g
b. 4.04 g
c. 8.08 g
d. 16.0 g
27. Use the equation to answer the question:
2A + B → A2B ∆H = -217.3 kJ
B + C → BC ∆H = -867.5 kJ
What is the value of ∆H for the reaction?
a. +1084.8 kJ
a. +1084.8 kJ
b. +650.2 kJ
c. -650.2 kJ
d. -1084.8 kJ
28. If 41.2 kJ of energy is needed to raise the temperature of 170.0 g of a liquid from 18.8oC to 65.2oC, what is the specific heat capacity of the solution?
a. 4.19 J/g.oC
b. 5.22 J/g.oC
c. 11.2 J/g.oC
d. 12.0 J/g.oC
29. Using the thermochemical equation, 2Al (s) + 3/2O2(g) → Al2O3(s), ∆H = -1676 kJ.
What is the ∆H of the following reaction: 2Al2O3(s) → 4Al(s) + 3O2(g).
a. -3352 kJ
b. -838 kJ
c. +838 kJ
d. +3352 kJ
30. When graphite and diamond burn, the reaction can be represented by the following thermochemical equation:
C(graphite) + O2(g) → CO2(g) ∆H = -393 kJ
C(diamond) + O2(g) → CO2(g) ∆H = -395 kJ
If 1.0 mol of graphite is converted to 1.0 mol of diamond under the same conditions, what is the heat energy change?
a. 2 kJ of heat are absorbed from the surroundings
b. 2 kJ of heat are given off to the surroundings
c. 788 kJ of heat are absorbed from the surroundings
d. 788 kJ of heat are given off to the surroundings
a. 4.19 J/g.oC
b. 5.22 J/g.oC
c. 11.2 J/g.oC
d. 12.0 J/g.oC
29. Using the thermochemical equation, 2Al (s) + 3/2O2(g) → Al2O3(s), ∆H = -1676 kJ.
What is the ∆H of the following reaction: 2Al2O3(s) → 4Al(s) + 3O2(g).
a. -3352 kJ
b. -838 kJ
c. +838 kJ
d. +3352 kJ
30. When graphite and diamond burn, the reaction can be represented by the following thermochemical equation:
C(graphite) + O2(g) → CO2(g) ∆H = -393 kJ
C(diamond) + O2(g) → CO2(g) ∆H = -395 kJ
If 1.0 mol of graphite is converted to 1.0 mol of diamond under the same conditions, what is the heat energy change?
a. 2 kJ of heat are absorbed from the surroundings
b. 2 kJ of heat are given off to the surroundings
c. 788 kJ of heat are absorbed from the surroundings
d. 788 kJ of heat are given off to the surroundings
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