What type of solution that contains all of the

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1 What type of solution that contains all of the solute it can hold at a given temperature? Saturated Solution

2 What type of solution that contains less solute than it is able to hold at a given temperature? Unsaturated Solution

3 What type of solution that contains more solute than it can hold at a given temperature? Supersaturated Solution

4 What is the term for a solution in which water is the solvent? Aqueous

5 What is the general rule for solubility? Like dissolves like

6 If a crystal is added to an aqueous solution and it causes many crystals to come out of the solution, what type of solution was it originally? Supersaturated

7 What term describes two liquids that can be mixed together but separate shortly after you cease mixing them? Immiscible

8 What term describes two liquids that are soluble in each other? Miscible

9 What is the substance that is dissolved in a solution? Solute

10 What is the substance that dissolves a solute to form a solution? Solvent

11 Does increasing temperature generally increase the solubility of a solid solute in a solvent? Yes, higher temps dissolve solids quicker

12 What is the effect on the rate of solution if the surface area of a solid is increased? More surface area = more solubility (EX Crushing, Cutting dissolves quicker)

13 When a gas is dissolved in a liquid, what factor will increase the rate of solution? More pressure (Soda with lid) Lower Temperature (colder = more gas dissolved)

14 Which factors listed below will speed up the dissolving of a solid solute in water? I. Cool the solution II. Heat the solution III. Grind up the solute IV. Decrease the surface area of the solute

15 A chemist is having some difficulty getting a yellow crystalline solid compound to dissolve in water. Which of the following strategies might she employ to increase the solubility of the solid? I. Crush the solid into a fine powder II. Heat the solution III. Stir the solution vigorously IV. Add ice to the solution

16 What are the products of a neutralization reaction between a strong acid and a strong base? Water and a salt

17 What type of acids and bases produce only a few ions in solution? Weak acids and bases

18 What type of solution contains more hydrogen ions than it does hydroxide ions? Acids/ acidic solution

19 What type of solution contains more hydroxide ions than it does hydrogen ions? base/ basic solution

20 What type of acid is nitric acid since it completely ionizes in solution? Strong acid

21 What is the molarity of a solution made by dissolving 17.0 g of lithium iodide (LiI) in enough water to make 500 ml of solution? M = mol/l 17.0g LiI X 1 mol LiI 133.8g 500 ml = L solution = mol LiI M = 0.127mol/0.500 L = 0.25mol/L

22 Calculate the molarity of a water solution of CaCl 2, given that 5.04 L of the solution contains 612 g of CaCl 2. M = moles/liter 612 grams CaCl 2 X 1 mol CaCl g CaCl 2 = 5.51 mol CaCl 2 M = 5.51 mol/ 5.04 L M = 1.09 mol/l

23 What would slow down the rate of a chemical reaction? Add an inhibitor Cooling Remove a catalyst

24 Which of the following will increase the reaction rate I. decrease in temperature II. increase concentration of the reactants III. increase surface area of the reactants IV. add an inhibitor

25 How does a catalyst increases the rate of a chemical reaction? It provides an alternative way for the reaction to have a lower activation energy

26 If 2.50 moles of potassium chlorate are used, how many moles of water would be produced? 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO H 2 O 2.5 moles KClO 3 X 11 mol H 2O 8 molkclo 3 = 3.4 mol H 2 O

27 How many moles of potassium chlorate are required to produce 18.0 g of water? 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO H 2 O 18.0 g H 2 O X 1 molh 2O 18 gh 2 O X 8 molkclo 3 11 mol H 2 O = 0.72 mol KClO 3

28 If 22.0 g of carbon dioxide are produced, how many grams of sugar (C 12 H 22 O 11 ) were used? 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO H 2 O 22.0 gco 2 X 1 moleco gco 2 X 1 molc 12H 22 O mol CO 2 X 342 gc 12H 22 O 11 1 molc 12 H 22 O 11 = 14.25gC 12 H 22 O 11

29 How many grams of sugar (C 12 H 22 O 11 ) were oxidized by the potassium chlorate, if 3.16 g of water were produced? 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO H 2 O 3.16 gh 2 O X 1 mol H 2O 18 g H 2 O X 1 molc 12H 22 O mol H 2 O X 342 gc 12H 22 O 11 1 molc 12 H 22 O 11 = 5.46 g C 12 H 22 O 11

30 Calculate the number of moles in 350.0g of potassium chlorate(kclo 3 ). 350 g KClO 3 X 1 mol KClO g KClO 3 = 2.86 moles KClO 3

31 Determine the molar mass of KC 2 H 3 O grams

32 Determine the number of moles in g Ag g Ag X 1 mol Ag g Ag = 0.24 mol Ag

33 How many atoms of Cu are in 3.00 moles? 3.00 mol Cu X 6.02 X mol Cu =

34 How many grams of CCl 4 are in 6.00 moles? The formula mass of carbon tetrachloride is g/mol mol CCl 4 X g CCl 4 1 mol CCl 4 = g CCl 4

35 How many moles are in 1.2 X molecules of water? 1.2 X 1024 molecules H 2 O X 1 mol H 2 O 6.02 X molecules

36 A reaction in which oxygen combines with a substance and releases heat and light can be classified as what type of reaction? Combustion Reaction

37 A reaction in which the atoms of one element replace the atoms of another element in a compound can be classified as what type of reaction? Single Replacement Reaction

38 The following reaction : AgNO 3(aq) + NaCl (aq) AgCl (s) + NaNO 3(aq) can be classified as what type of reaction? Double Replacement Reaction

39 The following reaction :2Hg + O 2 2HgO can be classified as what type of reaction? Synthesis Reaction

40 Given the following combustion reaction of a hydrocarbon, balance the equation and determine the coefficient of H 2 O. 2 C 4 H 6 + O 11 2 CO H 6 2 O

41 Balance the following equation. C 3 H 8 + O 5 2 CO H 4 2 O

42 What are the coefficients to correctly balance the formula equation? Cr 2 + Fe(NO 3 3 ) 2 Fe 3 + Cr(NO 2 3 ) 3

43 The following reaction : Cr + Fe(NO 3 ) 2 Fe + Cr(NO 3 ) 3 can be classified as what type of reaction? Single Replacement Reaction

44 The following reaction : H 2 O H 2 + O 2 can be classified as what type of reaction? Decomposition

45 What is the balanced equation when aluminum reacts with copper(ii)sulfate? According to reactivity series, Aluminum is MORE reactive than copper so it will replace it. 2 Al + CuSO Al 2 (SO 4 ) 3 + Cu

46 A compound contains 36.1 g calcium and 63.9 g chlorine. What is the empirical formula of the compound? 36.1 g Ca X 63.9 g Cl X 1 mol Ca g Ca 1 mol Cl g Cl = 0.90 mol Ca/ 0.90 = 1Ca = 1.8 mol Cl/ 0.90 = 2 Cl CaCl 2

47 A compound is composed of 82.68% mercury, (Hg), and 17.32% nitrogen, (N). What is the compound's empirical formula? g Hg X g N X 1 mol Hg g Hg 1 mol N g N = 0.41 mol Hg / 0.41 =1 Hg = 1.23 mol N / 0.41 = 3 N HgN 3

48 The elemental analysis of a sample of ionic compound gave the following results: 2.82 g Na, 4.35 g Cl, and 7.83 g O. The empirical formula of this compound is: 2.82 g Na X 4.35 g Cl X 7.83 g O X 1 mol Na g Na 1 mol Cl g Cl 1 mol O 16 g O = 0.123/0.123 = 1 Na = 0.123/0.123 = 1 Cl = 0.489/0.123 = 3.97 = 4 O NaClO 4

49 What is the molecular formula of a compound that is composed of 83.64% tin (Sn) and 16.36% phosphorous (P)? The compound's experimental molar mass is: g/mol g Sn X 1mol = 0.70mol = 1.3 Sn X 3 = 4 Sn 118.7g g P X 1mol = 0.53mol =1 P X 3 = 3 P 31 g 0.53 Sn 4 P 3

50 Find the percent composition of MgS. Mass of MgS = 56.4 g % comp of Mg = 24.3 X 100 = 43.1 % Mg 56.4 % comp of S = 32.1 X 100 = 56.9 % S 56.4

51 Find the percent composition of MgSO 4. Mass of MgSO 4 = g % Mg = 24.3 X 100 = 20.2 % Mg % S = 32.1 X 100 = 26.6 % S % O = X 100 = 53.2 % O

52 What is the percentage of chromium in BaCrO 4? Compound Mass = % Cr = X 100 = 20.5% Cr

53 What is the percentage of barium in BaCrO 4? Compound Mass = Barium = X 100 = 54.2% Ba

54 What is the percentage of oxygen in BaCrO 4? Compound Mass = Oxygen = X 100 = 25.3% O

55 If the pressure exerted by a gas at 25.0 o C in a volume of L is 3.81 atm, how many moles of gas are present? (Hint: R = L-atm/mol- K) PV=nRT = 298 K 3.81atm L = n (298 K) = n OR 6.85 X 10 3 moles

56 Calculate the volume that a mol sample of a gas will occupy at 265 K and a pressure of atm. PV = nrt atm V = mol K 0.900V = V = 7.81 L

57 Determine the Kelvin temperature required for mole of gas to fill a balloon to 1.20 L under atm pressure. PV = nrt (0.988atm)(1.20 L) = ( mol) (0.0821) T = T K

58 A sample of gas at 1.50 atm and 4.0 L is compressed to 2.5 L at a constant temperature. What is the new pressure? P 1 V 1 = P 2 V 2 (1.5atm)(4.0L) = P 2 (2.5L) 2.4 atm = P 2

59 A sample of gas at 313 K occupies a volume of 2.32 L. If the temperature is raised to 348 K what will be the new volume? V 1 T 1 = V 2 T L = V K 348 K = 313 V L = V 2

60 What is the final pressure in atm, if 5.25 L of gas at 75.0 C and 1.33 atm pressure is compressed to 2.75 L at 155 C? P 1V 1 T 1 = P 2V 2 T = 348 K = 428 K 1.33atm 5.25L 348 K = 957 P atm = P 2 = (P 2)(2.75L) 428 K

61 A sample of SO 2 gas has a volume of 9.50 L at a temperature of 320K. At what temperature will the gas have a volume of 2.55 L? V 1 T 1 = V L 320 K T 2 = 2.55 L T 2 (9.5L)T = K

62 What type of reactions release energy into its surroundings? Exothermic

63 What type of energy change is shown in the following reaction Sn +Cl 2 SnCl 2 DH= -325KJ Negative H = exothermic reaction

64 A 50.6 g sample of iron metal is heated from 19.7 o C to 24.3 o C. How many joules of heat will be absorbed? (specific heat of iron is (J/g o C) q = mc T q = (50.6g)(0.4494J/g o C)( ) q = Joules of heat absorbed

65 A sample of an unknown metal has a mass of g. As the sample cools from 90.5 o C to 25.7 o C, it releases 7020 J of energy. What is the specific heat of the sample? q = mc T T = ( )= J = (120.7g) C (-64.8) 7020 J = C C = -0.9 J/g o C

66 The specific heat of ethanol is 2.44 J/g C. How many joules of energy are required to heat 50.0 g of ethanol from C to 68.0 C? q = mc T T = 68.0 (-20.0) = 88.0 C q = (50.0g) (2.44J/g C) (88.0 C) q = 10,736 Joules

67 How much heat does it take to warm 16.0 g of pure water from 90 C to 100 C? The specific heat of water is 4.18 J/g C. q = mc T T = = 10 C q = (16.0g) (4.18 J/g C) (10 C) q = Joules of heat

68 How much heat does it take to warm g of pure water from C to C? The specific heat of water is J/g C. q = mc T T = = C q = (50.00g) (4.180 J/g C) (60.00 C) q = 12,540 Joules

69 The temperature of a sample of water increases from 20.0 C to 46.6 C as it absorbs 5650 J of heat. What is the mass of the sample? The specific heat of water is 4.18 J/g C. q = mc T T = = 26.6 C 5650 J = m (4.18 J/g C) (26.6 C) 5650 = m 50.9g = m

70 Predict the type of bond formed: Na + + Cl - NaCl Ionic

71 Predict the type of bond formed: Cl + Cl Cl 2 Covalent

72 Predict the type of bond formed between lithium and fluorine Ionic

73 Predict the type of bond formed between carbon and hydrogen Covalent

74 Predict the type of bond formed between copper and chlorine Ionic

75 Predict the type of bond between sodium and fluorine Ionic

76 Predict the type of bond between sulfur and oxygen Covalent

77 Given: nitrogen, sulfur, boron, or chlorine, which would tend to form an ion with a -3 charge? Nitrogen

78 Given: carbon, oxygen, barium, or potassium, which would tend to form an ion with a +2 charge? Barium

79 What is the charge of the phosphate in K 3 PO 4? 3-

80 What is the name of H 2 SO 4? Sulfuric Acid

81 What is the formula for copper (II) chloride? CuCl 2

82 What is the formula for aluminum sulfate? Al 2 (SO 4 ) 3

83 What s the correct formula for carbon disulfide? CS 2

84 What is the correct name for CCl 4 Carbon Tetrachloride

85 What is the correct name for MgSO 4 Magnesium Sulfate

86 What is the correct formula for (NH 4 ) 3 PO 4 Ammonium phosphate

87 What is the correct name of Li 2 CO 3 Lithium Carbonate

88 What is the correct name for NaOH Sodium Hydroxide

89 What is the correct formula for potassium permanganate KMnO 4

90 What is the correct formula for hydrochloric acid? HCl

91 What is the correct formula for phosphorous acid? H 3 PO 4

92 Predict the type of bond formed by sharing 4 electrons. Covalent (shared)

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided