Download Chemistry 1: Second Semester Practice Exam Read each question

Chemistry 1: Second Semester Practice Exam
Read each question and answer choice carefully. Choose the letter that best answers the question.
1. Which Kelvin temperature is equal to – 33 °C?
A. -33 K
C. 240 K
B. 33 K
D. 306 K
2. Which formula represents a mixture?
A. NH3 (aq)
B. NH3 (l)
C. NH3 (g)
D. NH3 (s)
3. As the temperature of a sample of an ideal gas increases at constant pressure the volume occupied by
the sample:
B. Increases
C. Remains the same
A. Decreases
4. Which sample of methane contains the greatest number of molecules at standard temperature?
A. 22.4 liters at 1 atmosphere
C. 11.2 liters at 1 atmosphere
B. 22.4 liters at 2 atmospheres
D. 11.2 liters at 2 atmospheres
5. At STP, 1 liter of oxygen gas would have the same number of molecules as
A. 1 Liter of H2
C. 3 Liters of CO2
B. 2 Liters of CO
D. 3 Liters of Ne
6. As the temperature of a gas increases with the volume remaining constant the pressure of the gas
A. Decreases
B. Increases
C. Remains the same
7. Under which conditions of temperature and pressure would a real gas be most likely to act as an ideal
gas?
C. Low temperature and high pressure
A. high temperature and high pressure
B. high temperature and low pressure
D. Low temperature and low pressure
8. How many significant digits are in the number 0.00120?
A. 6
B. 2
C. 3
D. 4
9. The pressure of 20 mL of a gas at constant temperature is changed from 4 atmospheres to 2
atmospheres. The new volume of gas is
A. 5 mL
C. 40 mL
B. 10 mL
D. 80 mL
10. Which may be heterogeneous?
A. A substance
B. An element
C. A compound
D. A mixture
11. As the pressure on a sample of a given gas increases at constant temperature, the volume of the gas
B. Decreases
C. Remains the same
A. Increases
12. In an experiment, the gram formula mass of magnesium was determined to be 24.7. Compared to the
accepted value of 24.3, the percent error for this determination was
A. 0.400
C. 24.7
B. 1.65
D. 98.4
For the following questions, match the chemical equation with the category that best describes it.
13. Single replacement D
14. Double replacement AC
15. Decomposition C
16. Synthesis B
17. Acid base AB
18. Combustion A
A. C10H8 + 12 O2 ---> 10 CO2 + 4 H2O
B. 2 H2 + O2 Æ 2 H2O
C. 2 KClO3 Æ 2 KCl + 3 O2
D. Mg + 2 H2O ---> Mg(OH)2 + H2
AB. HBr + NaOH ---> NaBr + H2O
AC. CuSO4 + Ba(NO3)2 Æ Cu(NO3)2 + BaSO4
Read each question and answer choice carefully. Choose the letter that best answers the question.
19. Put the following metals in order from most active to least active:
A. Copper, Iron, Calcium, Gold
B. Aluminum, manganese, tin, iron
C. Silver, Lead, Magnesium, Sodium
D. Potassium, Zinc, Nickel, Copper
20. Arrange the following list of reactions in order of most likely to occur to least likely to occur:
1. zinc added to a solution of copper (II) chloride
2. magnesium added to a solution lead (II) nitrate
3. nickel added to a solution of aluminum sulfate
4. copper added to a solution of silver nitrate
A. 2,1,4,3
C. 4,3,2,1
B. 3,4,1,2
D. 2,1,3,4
21. Will the following reaction take place? K + Pb(NO3)2 Æ
A. Yes
B. No
22. Will the following reaction take place? Pb(NO3)2 + KI Æ
A. Yes
B. No
23. The human body needs at least 1.03 x 10-2 mol of oxygen each minute. If all the oxygen is used for
the cellular respiration reaction shown below, how many grams of glucose does the human body
consume each minute?
C6H12O6(s) + 6 O2(g) Æ 6 CO2(g) + 6H20(l)
A. 11.1 g
B. 0.309 g
C. 0.31 g
D. 11.10 g
24. Given the reaction: 2KClO3 Æ 2 KCl + 3O2, What is the total number of moles of KCl produced
when 1.50 moles of potassium chlorate is decomposed?
C. 3.00
A. 1.50
B. 4.50
D. 0.750
25. Given the reaction: N2 (g) + 3 H2 (g) Æ 2 NH3 (g). How many liters of ammonia measured at STP are
produced when 28.0 grams of nitrogen are completely consumed?
A. 5.60
C. 22.4
B. 11.2
D. 44.8
26. What is the Molarity of a solution that contains 112 grams of KOH in 2.00 liters of solution?
A. 1.00 M
C. 3.00 M
B. 2.00 M
D. 4.00 M
27. A solution that has 20. grams of calcium bromide in 0.50 liters of solution has a Molarity of
A. 0.50
C. 5.0
B. 0.20
D. 10.
28. A 500 mL solution contains 10 grams of NaOH. The Molarity of this solution is
C. 0.25 M
A. 1.0 M
B. 0.50 M
D. 0.10 M
29. What mass of NaOH is needed to prepare 500 mL of an 0.50 M solution?
A. 10. grams
C. 25 grams
B. 20. grams
D. 40. grams
30. If 0.50 liter of a 12-molar solution is diluted to 1.0 liter the Molarity of the new solution is
A. 2.4
C. 12
B. 6.0
D. 24
31. Given the reaction: 2Na + 2H2O Æ 2NaOH + H2. What is the total number of moles of hydrogen
produces when 4 moles of sodium react completely?
A. 1
C. 3
B. 2
D. 4
32. Given the reaction at equilibrium: 2X(g) + 3Y(g) Ù 4Z(g). As the pressure on the system increases,
the temperature remaining constant, the amount of Z(g)
A. Decreases
B. Increases
C. Remains the same
33. Given the reaction A (g) + B (g) Ù AB (g). As the pressure increases at a constant temperature
the rate of the forward reaction will:
A. Decrease
B. Increase
C. Remain the same
34. Given the equilibrium reaction: A + B Ù C + D + heat. What change in the reaction system will
change the value of the equilibrium constant?
A. An increase in the concentration of A and B
B. An increase in the concentration of C and D
C. An increase in temperature
D. An increase in pressure
35. AgCl (s) Ù Ag 1+ (aq) + Cl 1- (aq). Consider this reaction at equilibrium. As chloride ions are
added to this system and the temperature is kept constant, the value of the equilibrium constant
A. Decreases
B. Increases
C. Remains the same
36. For the reaction A (g) + B (g) Ù AB (g), 1.0 mole of A and 1.0 mole of B are placed in a 1.0 liter
container. At equilibrium the concentration of AB is 0.20 M. What is the K for this reaction at a
constant temperature?
A. 0.64
C. 0.20
B. 0.25
D. 0.31
37. Given the equation CO (g) + 2 H2 (g) +heat Ù CH3OH (g). If 140. g of CO are added to 8.00 moles
of hydrogen, at equilibrium it is found that 2.50 moles of CH3OH are present in the 2.0 L container.
What is the equilibrium constant value?
A. 0.44
C. 4.4
B. 0.13
D. 2.3
38. Given the reaction A + BC Æ B + AC. Which are the reactants?
A. A and AC
C. A and BC
B. A and B
D. B and AC
39. Given the equation 6 ClO2 + 3 H2O 5 HClO3 + HCl . The mass of HClO3 produced when 4.72 g of
ClO2 reacts with 0.947 g H2O is 4.22 g. What is the percent yield?
D. 87.3
A. 86.5
B. 85.7
E. 81.3
C. 84.2
40. Given the equation 2 NH3 (g) + H2SO4 (g) Ù (NH4)2SO4 (g). 15.00 moles of NH3 and 10.5 moles of
H2SO4 were placed in a 1.50 liter flask and allowed to reach equilibrium. At equilibrium there were 6.00
moles of (NH4)2SO4. What is the Keq?
A. 0.0101
C. 0.0370
B. 0.333
D. 0.0909
41. A ___________ solution can only be produced if the conditions such as temperature and pressure
are changed.
A. Unsaturated
B. Supersaturated
C. Saturated
42. A solution which can not dissolve any more at the given temperature must be _________.
A. Unsaturated
B. Supersaturated
C. Saturated
43. If a crystal is added to a solution and it dissolves, it was _____________.
A. Unsaturated
B. Supersaturated
C. Saturated
44. Lemon juice and sugar are dissolved in water to make lemonade. The lemon juice is:
A. Solute
C. Sediment
B. Solvent
D. Suspension
Use the following solubility graph:
45. If 60 grams of sodium nitrate are dissolved in 100 mL of water at 55°C, the solution is said to be
A. Unsaturated
B. Supersaturated
C. Saturated
46. If 180 grams of potassium iodide are dissolved in a saturated solution of 100 mL of water, what
temperature must it be at?
A. 83 °C
B. 80 °C
C. 90 °C
D. 30 °C
47. Which change of phase is exothermic?
A. Gas to liquid
B. Solid to liquid
C. Solid to gas
D. Liquid to gas
48. As the pressure on a given sample of a gas increases at constant temperature the mass of the sample
A. Decreases
B. Increases
C. Remains the same
49. A sealed flask contains 1 mole of hydrogen gas and 3 moles of Helium gas at 20Û&,IWKe total
pressure is 400 torr the partial pressure of hydrogen is
A. 100 torr
C. 300 torr
B. 200 torr
D. 400 torr
50. At constant pressure the volume of a mole of any ideal gas varies
A. directly with the radius of the gas
C. Directly with the Kelvin temperature
D. Inversely with the Kelvin temperature
molecule
B. Inversely with the radius of the gas
molecule
51. Balance the equation written below. The coefficient in front of the O2 is
___ C2H5OH + __ O2 Æ __ H2O + __ CO2
A. 3
B. 5
C. 7
D. 9
52. A double replacement reaction is likely to occur when
A. a metal, such as zinc is placed in a concentrated acid
B. a hydrocarbon is burned in the presence of oxygen
C. a compound breaks down into its elemental components
D. two ionic compounds are dissolved in water
53. Which name is given to the reaction of a base with an acid to form a salt and water?
A. hydrolysis
B. hydration
C. neutralization
D. single replacement
54. How many moles of water will be produced if 40 moles of oxygen completely
reacts? 2 H2 (g) + O2 (g) Æ 2 H2O (g)
A. 10 moles
C. 40 moles
B. 20 moles
D. 80 moles
E. none of these
55. How many liters of hydrogen are needed to produce 20 L of methane, CH4 at STP?
C (s) + 2 H2 (g) Æ CH4 (g)
A. 2.0 L
B. 20 L
C. 22.4 L
D. 40 L