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Chemistry Practice EOC #1

1. If the solubility of ammonium chloride is 36.0 grams per 100 grams of water at 20.0°C, what is the maximum amount of this chemical that can be dissolved in 150 grams of water at 200°C?

A. 18.0 grams B. 36.0 grams C. 54.0 grams D. 72.0 grams

2. Many lakes in the midwestern part of the United States seem able to resist changes in pH caused by acid rain. Studies have revealed substantial amounts of limestone rock (contains CaCO3) in theses lakes. What is the limestone most likely doing for the water in the lake?

A. Increasing [OH-] B. Decreasing [OH-]

C. Increasing [H3O+] D. Decreasing [CO3-2]

3. Which statement best explains why oil and water do not mix?

A. One is miscible, and the other is immiscible.

B. One is polar compound, and the other is a non-polar compound.

C. Both are ionic compounds.

D. Both have different densities.

4. According to the balanced equation Zn (s) + 2HCl (aq) ( ZnCl2 (aq) + H2 (g), totally reacting 130 g of zinc with excess hydrochloric acid will release what mass of hydrogen?

A. 4.0 grams B. 6.0 grams C. 40 grams D. 65 grams

5. Which element is reduced in the following oxidation-reduction reaction?

HNO3 (aq) +I2 (c) ( HIO3 (aq) + NO2 (g) + H20 (I)

A. H B. I C. N D. O

6. What is the pH of a solution in which [H3O+] is 1 x 10-6 M?

A. - 6 B. 1 C. 6 D. 8

7.

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The energy diagram above describes which of the following facts about the reaction: 2AB ( A2 + B2?

A. The catalyzed reaction has too little energy to from the appropriate products.

B. The catalyzed reaction forms more products than does the uncatalyzed reaction.

C. The catalyzed reaction requires a lower activation energy than does the uncatalyzed reaction.

D. The catalyzed reaction forms fewer products than does the uncatalyzed reaction.

8. In what way do currently accepted models of the atom differ from the model in the drawing?

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A. Electrons do not have an elliptical orbit.

B. The nucleus contains only protons.

C. All electrons are the same distance from the nucleus.

D. Electrons do not have a negative charge.

9. Isotopes of an atom could be detected based on which of the following characteristics?

A. atomic radius B. nuclear charge C. nuclear mass D. number of electrons

10. What is the electron configuration for 3919K?

A. 1s22s22p63s23p63d1 B. 1s22s22p63s23p64s1

C. 1s22s22p63p64s24p1 D. 1s22s22p63s23p64s23d104p65s24d1

11. What is the formula for iron (III) oxide?

A. FeO3 B. Fe3O C. Fe2O3 D. FeO

The following graph shows solubilities of various salts in 100 grams of water at temperatures ranging from 0° C to 100 °C. Use the graph to answer questions 12 and 13.

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12. What mass of KCl is necessary to form a saturated solution if the KCl is dissolved in 200 grams of water at 50.0°C?

A. 21.0 g B. 42.0 g C. 55.0 g D. 84.0 g

13. If 90.0 grams of KNO3 were added to 50.0 grams of water at 50.0°C, about how many grams of KNO3 would settle out?

A. 0 grams B. 20.0 grams C. 45.0 grams D. 150 grams

14. If water is allowed to evaporate from an unsaturated saltwater solution, how will the concentration of the solution change?

A. The concentration will decrease.

B. The concentration will first increase, then decrease.

C. The concentration will remain the same.

D. The concentration will increase

15. In which system is the pressure in the test tube greater than atmospheric pressure?

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16. What is the rate of effusion of O2 (g) compared to CO2 (g)?

A. O2 effuses 1.38 times as fast as CO2. B. O2 effuses 1.17 times as fast as CO2.

C. O2 effuses 0.853 times as fast as CO2. D. O2 effuses 0.727 times as fast as CO2.

17. An ideal gas is confined to a 10.0 L balloon at STP. What is the new volume of the balloon when it is placed under 800 mmHg at 100°C?

A. 14.4 L B. 13.0 L C. 7.70 L D. 7.00 L

18. What is the shape of a molecule, which has two shared pairs of electrons and no unshared pairs?

A. tetrahedral B. bent C. trigonal planar D. linear

19. The following data was collected during an experiment.

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Which of the following statements contains a correct explanation of the observed data?

A. The conductivity of solution B and its low freezing point are a result of more ions being released in the solvent by the solute.

B. The freezing points of solutions A and C are nearly the same because they contain solutes that do not dissolve well.

C. The conductivity of A is slight because, being an acid, it is a strong electrolyte.

D. The relationship between freezing points and conductivity cannot be explained without more data.

20. A substance dissolves well in water but not in benzene. Which of the following can be concluded about the substance?

A. The substance may be either polar or nonpolar.

B. The substance is nonpolar.

C. The substance is polar.

D. The substance is neither polar nor nonpolar.

21. When bonded with sulfur, which element will most likely form an ionic compound?

A. oxygen B. calcium C. hydrogen D. chlorine

22. Which of the following pairs of substances will mix to produce a solution that can conduct an electric current?

A. Sodium chloride (NaCl) and benzene (C6H6)

B. Iodine (I2) and benzene (C6H6)

C. Benzene (C6H6) and water (H2O)

D. Lithium nitrate (LiNO3) and water (H2O)

23. A violent reaction occurs when sodium is placed in water. Which element would produce a similar reaction with water?

A. Mg B. S C. K D. Cr

24. An element with the electron configuration [Ne] 3s23p2 would be expected to react similarly to which of the following elements?

A. aluminum B. carbon C. phosphorus D. neon

25. A student placed a strip of copper in a container of iodine vapor. A chemical reaction occurred that produced a white powder on the strip of copper. The following data were collected:

Experiment Results

Original mass of copper strip 28.96 g

Mass of copper and white powder 30.38 g

Final mass of copper strip 28.60 g

How many moles of copper were in the original strip?

A. 0.4557 mole B. 2.194 moles C. 1840 moles D. 6.020 x 1023 moles

26. How many moles of sodium carbonate are in 500 mL of a 0.300 M solution of sodium carbonate?

A. 0.150 mole B. 0.840 mole C. 3.18 moles D. 150 moles

27. The product contains copper (II) ions; which of the following is an acceptable balanced equation for this reaction?

A. Cu2 (s) + I2 (g) ( 2CuI (s) B. Cu (s) + I (g) ( CuI (s)

C. Cu (s) + I2 (g) ( CuI2 (s) D. 4Cu (s) + I2 (g) ( 2Cu2I (s)

28. Butane (C4H10) is used as the fuel in many portable lighters. When butane is completely combusted in oxygen, what is the coefficient for the water produced in the properly balanced equation that represents the reaction?

A. 10 B. 8 C. 6 D. 4

29. Consider the following balanced equation: 2KClO3 (s) ( 2KCl (s) + 3O2 (g)

How many moles of O2 will be obtained by decomposing 3.50 moles of KClO3?

A. 5.25 moles B. 3.00 moles C. 2.30 moles D. 0.530 mole

30. Consider the following balanced equation: 5CO + I2O5 ( 5CO2 + I2

Which substance is the oxidizing agent?

A. CO B. I2O5 C. CO2 D. I2

Use the graph below to answer questions 31 – 33.

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31. In the graph, which of the following is represented by the letter L?

A. reaction heat B. progress of reaction C. catalytic effect D. activation energy

32. The reaction represented in the graph is best described by which of the following terms?

A. unreactive B. nonreversible C. exothermic D. endothermic

33. On the graph, which dimension would be changed if the rate of reaction were to be altered by a catalyst?

A. K B. L C. N D. O

34. How can the reaction rate be increased for a reaction between hydrogen gas and chlorine gas?

A. Increase the size of the container.

B. Decrease the temperature of the reactants.

C. Decrease pressure on the molecules of the reactants.

D. Increase the concentration of either or both reactant molecules.

35. What volume of 0.2 M potassium hydroxide (KOH) is needed to neutralize 40 mL of 0.2 M sulfuric acid (H2SO4)?

A. 20 mL B. 40 mL C. 80 mL D. 160 mL

KEY

1. C 21. B

2. A 22. D

3. B 23. C

4. A 24. B

5. C 25. A

6. C 26. A

7. C 27. C

8. A 28. A

9. C 29. A

10. B 30. B

11. C 31. D

12. D 32. C

13. C 33. B

14. D 34. D

15. D 35. C

16. B

17. B

18. D

19. A

20. C

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