AP Chemistry 1st Semester Final Review Name:____________________ 2015-2016 Page 1 A) CO2 B) C3H6 C) CH3Cl D) N2O3 E) SiO2 1. Which of the following contains only sigma ( s) bonds? A) B) C) D) 2. What is the equilibrium law expression for the above reaction? A) [CO] and [CO2] both increase B) [CO] and [CO2] both decrease C) [CO] increases and [CO2] decreases D) [CO] decreases and [CO2] increases E) [CO] decreases and [CO2] remains constant 3. H2O(g ) + CO(g ) H2( g ) + CO2( g ) A closed container is initially filled with H 2O and CO. As the reaction proceeds towards equilibrium the A) Activation energy is not required. B) The addition of a catalyst does not change equilibrium concentrations. C) Changes do not occur at the microscopic level. D) Two opposing reactions occur at the same rate. E) Temperature and pressure affect the equilibrium position equally. 4. Which of the following is characteristic of all systems at equilibrium? A) 1.0 moles B) 2.0 moles C) 3.0 moles D) 4.0 moles E) 5.0 moles 5. H2O(g ) + CO(g ) H2( g ) + CO2( g ) Initially 5.0 moles of H2O and 4.0 moles of CO were reacted in the system above. At equilibrium, it is found that 2.0 moles of H 2 are present. How many moles of H2 O remain in the mixture? 6. Base your answer to the following question on the equation and the choices provided. CN – ( aq )+H2O(l ) « HCN( aq ) + OH – ( aq ) (A) increases (B) decreases (C) remains the same (D) increases, then decreases (E) decreases, then increases A) A B) B C) C D) D E) E If the pressure is increased, the [OH – ] A) 2 NO( g ) « N2( g )+O2( g ) B) 2 H2( g ) + O2( g ) « 2 H2O(g ) C) 2 NH3( g ) « N2( g )+3H2( g ) D) 2 CO2( g ) « 2 CO( g )+O2( g ) E) 2 SO3( g ) « 2 SO2( g )+O2( g ) 7. When at equilibrium, which reaction shifts to the right if pressure is increased?
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AP Chemistry 1st Semester Final Review Name:____________________2015-2016
Page 1
A) CO2 B) C3H6
C) CH3Cl D) N2O3
E) SiO2
1. Which of the following contains only sigma (s) bonds?
A)
B)
C)
D)
2. What is the equilibrium law expression for the abovereaction?
A) [CO] and [CO2] both increaseB) [CO] and [CO2] both decreaseC) [CO] increases and [CO2] decreasesD) [CO] decreases and [CO2] increasesE) [CO] decreases and [CO2] remains constant
3. H2O(g) + CO(g) H2(g) + CO2(g)
A closed container is initially filled with H2O and CO.As the reaction proceeds towards equilibrium the
A) Activation energy is not required.B) The addition of a catalyst does not change
equilibrium concentrations.C) Changes do not occur at the microscopic level.D) Two opposing reactions occur at the same rate.E) Temperature and pressure affect the equilibrium
position equally.
4. Which of the following is characteristic of all systems atequilibrium?
A) 1.0 moles B) 2.0 molesC) 3.0 moles D) 4.0 molesE) 5.0 moles
5. H2O(g) + CO(g) H2(g) + CO2(g)
Initially 5.0 moles of H2O and 4.0 moles of CO werereacted in the system above. At equilibrium, it is foundthat 2.0 moles of H2 are present. How many moles of H2O remain in the mixture?
6. Base your answer to the following question on theequation and the choices provided. CN–(aq) + H2O(l) « HCN(aq) + OH–(aq) (A) increases (B) decreases (C) remains the same (D) increases, then decreases (E) decreases, then increases
7. When at equilibrium, which reaction shifts to the right ifpressure is increased?
1st Semester Final Review
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A)
B)
C)
D)
8. N2(g) + 3 H2(g) 2 NH3(g) + 22 kcal
Which shows what happens to the concentrations of thethree gases when some NH3 is removed from the aboveequilibrium system with temperature and pressureremaining constant.
A) amount of AgCl(s) increasesB) rate of forward reaction decreasesC) concentration of Cl–(aq) increasesD) concentration of Ag(S2O3)23–(aq) decreasesE) equilibrium cannot be reestablished
Which change to the above system at equilibrium willincrease the concentration of Br2(g)?
A) A decrease in the total pressureB) A decrease in the concentration of H2(g)C) An increase in the volume of the reaction chamberD) A decrease in the temperature of the reaction
chamberE) A decrease in the concentration of N2(g)
12. N2(g) + 3 H2(g) 2 NH3(g) + 24 kcal
Which change will increase the above equilibriumconcentration of ammonia, NH3?
A) 0.15 B) 0.94 C) 1.5 D) 1.6 E) 9.4
13. At equilibrium, represented by the equation below, the[NO] is 2.0 M; [O2] is 3.0 M; [N2O5] is 8.0M.
4 NO(g) + 3 O2(g) 2 N2O5(g) + Heat
What is the numerical value of the equilibriumconstant, K, at this temperature?
A) 9.0 moles/liter B) 2.0 moles/literC) 3.0 moles/liter D) 4.5 moles/literE) 6.0 moles/liter
14. I2(g) 2 I(g) K = 9.0 moles/liter
At equilibrium, the concentration of I2 is 1.0 mole/liter.What is the concentration of the I at this temperature ifthe system behaves according to the above equation?
1st Semester Final Review
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A) area I onlyB) area IV onlyC) areas II and III onlyD) areas I, II and III onlyE) areas I and IV only
15. The relative number of molecules with a given kineticenergy is plotted against kinetic energy. An uncatalyzedreaction with an activation energy, Ea, is beingconsidered. In which region of the above kinetic energydistribution graph will all collisions result in a chemicalreaction?
Base your answers to questions 16 through 21 on thediagram shown below.
A) 1 and 6 B) 2 and 3C) 3 and 4 D) 4, 5 and 6E) 3 and 6
16. A catalyst would change
A) 1 B) 2 C) 3 D) 4 E) 5
17. Which represents the heat of reaction?
A) 1 B) 2 C) 3 D) 4 E) 6
18. Which represents the activation energy for the forwardreaction?
A) 6 B) 2 C) 3 D) 4 E) 5
19. Which represents the energy of the activated complex?
A) 6 B) 2 C) 3 D) 4 E) 5
20. The products have an energy represented by number
A) reactantsB) productsC) activated complexD) endothermic reaction
21. The least stable species in this diagram is the
22. Potassium sulfide is completely ionized in water:K2S(s) ® 2 K+(aq) + S2–(aq) Which of the followingequations is true?
A) [Sr2+] = 0.12 M and [OH–] = 0.12 MB) [Sr2+] = 0.12 M and [OH–] = 0.24 MC) [Sr2+] = 0.090 M and [OH–] = 0.090 MD) [Sr2+] = 0.090 M and [OH–] = 0.180 ME) [Sr2+] = 0.090 M and [OH–] = 0.24 M
23. When 250. mL of 0.36 M Sr(OH)2 are added to 750.mL of water, the resulting ion concentrations are
26. The element X forms diatomic molecules with each ofthe elements P, Q, S, T.
Based on the table above, which lists the compounds inthe order of increasing ionic character?Lowest Highest
A) Ionic B) MetallicC) Network covalent D) Molecular covalentE) Coordinate covalent
27. A certain solid is insoluble in water, does not conductelectricity in either the solid or liquid state and melts ata temperature above 1500°C. Which type of bonding ismost likely between lattice points in its crystallinestructure?
Base your answers to questions 28 through 30 on thefollowing bonding types.
66. Which of the following reactions has the largestincrease in entropy?
A) II and IV B) II and IIIC) I and III D) I and IVE) I and II
67. According to the table above, which reactions occurspontaneously?
A) AB) BC) CD) DE) All compounds can be formed spontaneously at
298K
68. According to the table above, which compound cannot be formed spontaneously from its elements at 298 K?
A) 5.02 × 10–5 B) 34100C) 0.00003 D) 0.0782 × 10–3E) 32312 × 1052
69. Which number contains exactly 5 significant digits?
A) 7.2047 g/mL B) 7.205 g/mLC) 7.20 g/mL D) 7.2 g/mLE) 7 g/mL
70. A student calculated the mass of a small piece ofunreactive metal. This piece of metal was added to apartially filled graduated cylinder. The followingmeasurements were made by the student:Mass of metal = 13.689 gramsVolume of water before the metal was added= 7.51millilitersVolume of water after the metal was added= 9.41millilitersThe density of the metal should be reported as