Name Period

Multiple Choice Final Exam Review Honors/Gifted Chemistry

The Mole

1. Determine the molar mass of sulfuric acid. liaSOlt Sa i-Cv-V- L Csit4-1(:te S 30{-4-G (SO421) 2. How many moles are in 100.0 g met anol, CH3OH?

100Den >c -3. (-z.SK-0-e_ 3. 3-c' Calculate the number of atoms in ea h of the following.

a) 2.15 ma Oles,gold, Au v (0 .02-7, 0'3

`' 1 ■.,..- b) 25.8intexcnry, Hg - 0 ix

RD 0 4. What is an empirical formula?

10--ta 5. Determine the empirical formula for each of t ollowing:

a) Hydrogen peroxide, ( b) Hexane, C61114

6. One of the substances in a new alkalin ery is composed of 63.0 g manganese and 37.0 g oxygen by mass. Determine the empirical formula of the compound in the battery. (03,0 Mit x 5Y 9 = I . s- /14.. Vt. (41s-

31' DI 2- ' 3 12-5;"--4-A,114-1S- - 015

7,-11-1 XI 01-2- eve "A---k

I h a C____&vv-e Cokfrtc rr...Alos

Chapter 1Q

" TO

Stoichiometry Chapter 11

7. What is stoichiometry? rl WI ye- re,Zstis

t, a_ Ckti.v.ALe' ( n try,‘ +Le L24.4.,) n, Cow ab /tA.W• 8. What law governs balancing equations and, ultimately, stoichiometry?

Louth) -e e_c7v,--4-eft v 9. When solid copper is added to nitric acid, copper(II) nitrate, nitrogen dioxide, and

water are produced. Write the balanced chemical equation for the reaction. List six

mole ratios for the reactions. CAL N 0L,(No3 z at.locz +x-120

lv,tecti = 4v,v4 ,e v.) oa_ : *111,54 CL, L-vv-f-e 'N 000 CkAM'1(3-)2_ 4 ho-t CAA. ■ .A54-- tte 0 le (4 63 2-w".€ t42-

10. When an antacid tablet dissolves in water, the fizz is due to a reaction between sodium hydrogen carbonate (sodium bicarbonate, NaHCO3) and citric acid (H3C6H507).

3NaHCO3(aq) + H3C6H507(aq) —> 3CO2(g) + 3H20(1) + Na3C6H507(aq) How many moles of carbon dioxide can be produced if one tablet containing 0.0119 mol NaHCO3 is dissolved?

• 0 1(6/ wk,'"(- IJAUS ej)2- , 2-

19. What is the rule for dissolving? VAct ssbUre.4-.), t I

s -k- 25 Oz \Naz i. lgNaO

Period

e, m ot.{-4-e r Rcwt .

15. What is the formula used for calculating percent yield?

produced, what is the percent yield?

„cot ft-cA- D Ex. p

(00.03 100

TT, - c_t 4 X, [0 o

16. Pure zirconium is obtainecFusing the two-step Van Arkel process. In the first step, impure zirconium and iodine are heated to produce zirconium iodide (ZrI4). In the second step, ZrI4 is decomposed to produce pure zirconium.

ZrI4(s) -> Zr(s) + 2I2(g) Determine the percent yield of zirconium if 45.0 g ZrI4 is decomposed and 5.00 g pure Zr is obtained.

1,4 g(-23 = CI

Solutions Chapter 14 17. What is the difference between solute and solvent? Identify the solute and solvent in

a sugar-waer solution. L 6-i-91 l_., out; +1 4.1 ,2 if f,c;v4,L 4 t ve..4,,t ttisseeveci Aucebt u .4.9

18. Explain the difference between saturated, unsaturated and supeNaturated.

ctlu-t-i mcuti exb St-G-1a -it • CSAA•t- Sti

s.56tve rkal'e

11. Carbon dioxide is released into the atmosphere through the combustion of octane (C8H18) in gasoline. Write the balanced chemical equation for the combustion of octane and calculate the mass of octane neededo release 5.00 mol CO2.

5"

©0 v,A,C) Ak- I-I tS & WI. 2- -_-_ 7/./- eg ti-ts z x IG Of-e-a.a.,_ lot g 12. Ammonium nitrate (NH4NO3), an important fertilizer, produces 20 gas an

when it decomposes. Determine the mass of water produced from the decomposition of 25.0 g of of ammonium nitrate. NI-Li-WO ,--4 1■1 20 4 *2 2., 0

, --"•• -----. 13. at is meant b y limiting reactant?

.S Vxces/ reactant.

(-.._ r um 0 u.i- rs+ 6.; ,,,,is proms--t4& 14. Photosynthesis reactions in green plants use carbon dioxide and water to produce

glucose (C6H1206) and oxygen. Write the balanced chemical equation for the reaction. If a plant has 88.0 g carbon dioxide and 64.0 g water available for photosynthesis, determine the limiting reactant and the maximum mass oflucose produced. 6

epz N Co 4- C‘, Ha_ 4.

61"),5 1/41° k A. C2O'"A vgi wee 1‘4,0V tes p 4-re tom.

-if this process occurs (with the amounts listed above) and 54.0g of ue •

5 , Clea tuu

r

Sti

20. What is a polar molecule? (e, ptist -hs v-e. ciL.A,tt

21. What is the most common polar solvent?

trizta AA-Le 40

° ekci.x bha coy ed2g.4-1, ct,"

60k-e-ti

Name Period

22. Predict if the following substances are soluble or insoluble in water: • Ionic compounds Ste` (-- V4JL4i) • Hydrocarbons .\‘,.-Srs-6,1-e-e.. (vk.o.f...vo-trAirN) • Sugars S (IRAA-b-et-. (9 'f-fi-.'r • Diatomic molecules k tA. d-eu13-4... VCV7wki"...-PAA)

23. What happens to the solubility of solids as temperature increases? Gases? K

24. A small crystal of solute is added to a solution. For each scenario listed below, determine what can be concluded about the ori rinal solution.

a) The crystal dissolves b) The crystal settles to the bottom sAttA c) The crystal causes a large amount of precipitate to form

25. What is a colligative property? VCO-VAr-t'e--4-) ( ,c

-k-D 41,v4_ tta-4-441-) 41) a Urtu---U 41112 Mar ‘`b 26. Calculate the percent by mass o NaCl dissolved in 88.6 water. 1.-ke

3 . -s- .S -:-.-. 27. What is the molarity of the following solution?

qsAct3Lteic 9

a) 1.35 mol H2SO4 in 2.00 L of solution 1 • a Doi_

I j ,R_ gg3 x k." , 03(1

o as

F

svP KV

•■•11. 00.*

Ce,(504),

10 20 30 40 50 60 70

Temperature (t)

03

Acids & Bases Chapter 18 32. According to Arrhenius, acids donate car.. ions in solution, while bases

donate VIAO-00x...Ck-e- ions in solution. 33. According to the Bronsted-Lowry model of acids and bases, acids are considered

hydrogen (VD-Vu) s. and bases are hydrogen Jos.

150

140

130

120

110

100

90 80

70

60

50

40

30

20

10

Oo

b) 2.48 g CaF2 irt 375 mL of solution

• 3 s- L 28. At 90°C, 10 g of potassium chlorate is dissolved in

100 g of water. Is this solution saturated, unsaturated or supersaturated?

29. How many grams of sodium nitrate eeded to saturate 100 g of water at 10°C?

30. If 12g of solute are needed to saturate 11 1 g of water, how man grams of solute would be needed to saturate 30g of water? .2.

3 ° 31. Which substance shows tgeDlarges increase in 80 90 solubility as the temperature is increased? 100

Name Period

34. Identify the conjugate a*d-base pairs in t a) HCOOH(aq) + f120(1) 4-÷

A

llowing equations. HC00-(aq) + 4,1130±(aq)

c b) NH3(aq) + H20(1) <-4 NH4+(aq) + OH-(aq)

Ut) 35. Acids taste StWer and bases taste ‘10 4e-1r' . 36. Acids have a pH range from 0 — 6.91 , with 0 being the strongest. Bases have

a pH range from 1.01 - 14 , with 14 being the strongest. 37. Distinguish between a strong acid/base and a weak acid/base.

s' 8n fhi-GLS or- 61i.,LSOcklo-tt. tO 0 t) Which would cause a light bulb to glow more brightly? \1•1-e-0-1 ,̀

38. Name the ollowing substances and indicate whether they are an acid or base. a) HC1 b) NaOH t?)0.4-e- c) H3PO4 A-Liz- d) Mg(CID2

39. An aqueous solution tastes sour and turns litmus red.

40. pH + p0H 41. What is a neutralization reaction? 42. Predict the products of the following neutralization reaction:

H2SO4 + NaOH -> -V Z-D + i\I a 2... SC)i-i 43. In a titration 33.21 mL of 0.3020M rubidium hydroxide solution is required to exactly

neutralize 20.00 mL hydrofluoric acid solution. What is the molarity of the hydrofluoric acid solution? ft c --V k boil --sit 1-k 20 -t- R. 10 F

oa-i3, wk. 7-. __x-- x _ . 0 ( Do 4,,,,,..t B uw.. x 1 4 - p 1 0 tp‘ A,9.k. flf v 4. 2- ''.- p (a 4.4-0,

44. If an acid has a [1-1+1 = 1.2 x 10-4 M, determine [OW pH and OH. v 02 0 L pit =-10 1 . 24, ■ a- 4, I LI— 3 '5 ..- PD K :. W"

5,3 xlb -IINt = solution as a pH of 10. It would be 1 0 00 times more

basic) than a solution with a pH of 7.

46. What is the relationship between [111 and [OW] for a) An acidic solution? at-4-3 > Co IA 2 b) A basic solution? Ept-t--2 > c) A neutral solution?

47. What is specific heat? What is this value for water?

tIANLOAAN± vusr-61 ^LA-AA ri4,414. 441A 1414.bs ° 48. What is the formula for calculating heat gained/lost in a chemical reaction.

cf y•f\

s-A „&„tf "\-.4. 1z

Is the solutio acidic or basic?

+ Gaia-a * Irk 0

acidic or

Reaction Pathway

56. Draw an energy diagram for an exothermic reaction. Label /A parts. Pkift"

57. What is entropy?

-\) S Odftr- (aCt..0..S

Name Period

49. Explain the difference between exothermic and endothermic reactions.

re-ez_v.4/24, it-oir?-s ot-a

50. In which type of reaction is energy a reactant? In which type is energy a product?

51. If q or AH is "+", the reaction i endo exo. If q is "—", the reaction is endo 52. How much heat is absorbed by a 100 g sample of granite as energy from the sun

causes its temperature to change from 10°C to 29°C? The specific heat of granite is

6$o 375.,cz_q = 30-51y

53. The temperature of a piece of copper with a mass of 95.4 g increases from 25.0°C to 48.0°C wh n the metal 849 J of heat. What is the specific heat of copper?

gi.A.q -3—.= ctc- 4 ..--:-_

54. A piecey„

of me

0.803 J/g.°C.

+3.0 — 0 0C.,)

23 grams is heated to 100.0°C and dropped into 35mL of water at 15.0°C. If the final temperature of the lead and water is 18.2°C, what is the specific heat of the metal?

291 2 r ' 233 ( 106 55. Use the graph below and determine the activation energy and the AH for the forward

reaction. Is the process endo or exothermic?

Potential Energy

6a)

EA

= Ras--

ENDO

d) When will this reaction be spontaneous?

61. When will the following reaction be spontaneous and why? Co(s) + S(s) + 2O2(g) CoSO4(s) AH=-888.3 kJ/mol

cnt Aeivi ,

Name Period

58. Identify the name of the following phase/state changes and label each as exothermic or endothermic.

Process Name of

Phase Change

Endothermic or Exothermic

Change in entropy AS

Positive or negative

1. C3H8 (g) ---> C3H8 (1) C-014Q41saki,N.. c,,,,,.)1/4. 0

2. CO2 (s) ---> CO2 (g) 5W,i ,c,li o-,&- 6-4- O + 3. CioH8 (s) ---> C1oH8 (1) (*ail*t3 €4". 1.0 ± 4. 1120 (1) ---> H20 (s) -4,ee I:. 4.1 0

59. Use the heating curve below to answer the lowing questions.

a. What phases are present at each segment? b. Where is kinetic energy increasing? I I 3 j 5- c. What is the melting pt? O ° C d. What is the boiling pt? 10 0 °C- e. Where is potential energy increasing?

60. 2C.Il1o(g) + 402(g) 4 10H20(g) + ICO2(g) + 7018 kJ a) How much heat is released if 23.0 grams of butane () is rn

o 1 g kr R3 ‘01 x .

4

b) If 176 kJ of heat are8

released, how many grams of butane were

52111r. burned? h 6 KT

c) What is the sign of All? — What is the sign of AS?

c41° CActo*Ate"'

13 %-irst.e

6 IA' • rxki A afre_

Name Period

Kinetics & Equilibrium Chapter 16-17

62. List the three states of matter in order of increasing molecular motion.

< 63. Describe the arrangement of particles in a:

a) solid. VlovrA4' - ,--Keitt y-ta-<-4A — b) liquid. -c-ia \ c) gas. ‘6_ 0 s

64. List four ways to increase the rate of a reaction. o VIC

Sur -C-9.-c.e e_ CIPKW•kStsezt--+;1"A-4 • 't C

65. How/do you increase the surface area of a substance?

QA/ e)wat.12-Q.eir

66. What is a catalyst? How does a catalyst work? L-4 r-u3i-- lek ; cLe.* vo.sh a-A.d

67. Write a rate law that is 2nd order with res ect to [A] and 1st order with respect to [B]. et:1 2 ig

a) If both [A] and [B] are tripled, what happens to the rate?

68. Use the following data to determine the rate law for the reaction aA + bB -> products.

Experimental Initial Rates for aA + bB —3 products

Trial Initial [A] (M)

Initial [B] (M)_.,\

Initial Rate (mol/(14.$))

1 0.100 Z 0.100 , 2.00 x 10-3 2 0.200 .> '0.10 4.00 x 10-3 / 3 ( 0.200. 0.200 16.0 x 10-3 ,

fielt,a4 e-v‘ a. g‘30e4i.-- Q 71. If pressure on a gaseous system is increased, which way will the system shift. %-e-V e

-tke c-Adti2 v./44w Le /144- nutst-eu , 72. If temperature of a system in increases, which w

etAk".- Al^-e LILAkle4-aA0

—R9AA----12/1a9-e-Ar % 6,61:0 kAni f,,,,16 Els 14\) -4s/11

vo..4„cet. dt-ek, 6̀(4P-12-4-

apt oeu-v-e- or veret,,,,,

0 't PVC

69. What is chemical equilibrium? A- giVe_12z:e VAL '60,\ r;v,

70. State LeChatelier's Principle.

SIV`e.°44•' will the system shift?

as re4Laci,v,4-- ("ok 62-f34)

Name Period

73. Use LeChatelier's principle to predict how each of the following changes would affect this equilibrium? How would this change the concentration of H2?

H2(g) + CO2(g) 4-> H2O(g) + CO(g) + heat L a) Adding H20(g) to the system 1 el

b) Removing CO(g) from the system 4e- a c) Increasing the temperature of the system I

KI G d) Decreasing the pressure of the system tja cla_vvy_, (5a-4'v-Q-42re-40

% TA< 0-Y‘ AolthL, fs• Clad)

a) At equilibrium [I12] = 0.100 M, [CO2] = 0.0200 M, [H2O] = 0.025, and [CO] = 0.00032 M. Calculate Keg.

Da-so E. 03 °°03.23 oo

c't] C-'13 b) Now that yo th equil rium constant, calculate the molarity of H2 if [CO2] = 0.0800 M, [H2O] = 0.0070, and [CO] = 0.002 M

74. Use the balanced equation from the question above to answer this question.

0040 Cool .Dol- , OIfLt- 08) vv"--)

Gases Chapter 13 75. What temperature scale has absolute zero as its starting point?

76. What is the value of absolute zero? What happens to molecular motion at this temperature?

77. How is Celsius converted to Kelvin? What is -65°C on the Kelvin scale?

K = aog 78. Complete the following table involving as laws.

Gas Law Variables Involved

Mathematical Equation

Direct/Inverse Relationship

Example

Boyle's Law p y PI 1)2 va Tr1/414)•

51ktezticv. Charles' Law \/ T vi_ \i,....

I I 1.-z_

baipt5-Y, d)(ek

Gay- Lussac's

Pi i T' - _ P2-,4 f- I I 1 2.

9 -.- -1) - reeA- INA A'aine.1 Combined Gas Law

p v T

V( VI I72 Va-

--..t..-7— .7.--

‘ 1 —1- 2— Ideal Gas Law (Avogadro)

v v, ...r nko tR,0

\i IA KT \t",. ..-r- 22 . 4 L

Graham's Law

MICAL-4 1 s5 4.. ast41/4 \

-;-:, to cf\x/ I ,r3

Koteu.-Qto /r1' ML

9miSfix-s-

Pk/

VNAtses i-C--fv40-e- 0 r -tc-fv1/44-e- t,

\-ke_ 044> Co,_

Pv,

= P2-47- 79• A sample of oxygen gas occupies a volume of 250. mL at 740 torr pressure. What

volume will it occupy at 800. torr pressure? (q Li -0 )(2.5t,) ____ (c 0 b)0c X= 231

80. A sample of nitrogen occupies a volume of 250 mL at 25°C. What volume will it occupy at 95°C? 2._50 ...., ........ )( ,------ 309 29 gs - 368

81. The pressure in an automobile tire is 1.88 atm at 25.0°C. What will be the ressure if the temperature warms up to 37.0°C? \ is g x --r= I . 9 (.0 cd-vv

a98 3 l b

82. A sample of nitrogen gas is stored in a 500.0 mL flask at 108 kPa and 10.0°C. The gas is transferred to a 750.0-mL flask at 21°C. What is the pressure of nitro en in the second flask? 008)(c•Do X 7Si%)

• LA 83. 1 mole of any gas will occupy L at STP. 2e 2. ct 4 84. Carbon monoxide, CO, is a product of incomplete combustion of fuels. Find the

volume that 42 g of carbon monoxide gas occupies at STP. 42- 9 X I 't v .P.Vi L .7. 3 G = 13 14, L'

,

g,'g j ' --77-,...0.<7 ' 85. What volume will 2.0 moles of nitrogen occupy-at-720 mmHg and 20°C?

X - ii7.- 49 Lill l„ 0 tOXV• = (-)(' "2-1)(2-9 3) ew‘ --12. 0 ,v-1,-.4

86. When iron rusts, it undergoes a reaction with oxygen to form iron(III) oxide. Calculate the volume of oxygen gas at STP that is required to completely react with_ 52.0 g of iron. Li, fe., 4- 30 a, ---. a•Fe. O3

c.e.14- 02. - 62.03 2 1..... ,,, / ibs.s.k. 3,,e0,... (;1 14('

& sif 52 , ....5 ic, , . ...........-. t, ...______ __ x

)( 55.8 i bt Fe I 87. What is the volume of 4.5 grams of chlorine gas at STP?

oj cA, „ >c A

230

gas (C3H8)? Assume constant conditions.

. 00 L Rce 5 L Oz

A f L e3 h Q 2

0,r (-k-te_

eovit..,

44, 0 3/4, tkt4)t vAxh- .

44,t_ Ins. Lgit..

Name Period

•

88. What volume of oxygen gas is needed for the complete combustion of 4.00L propane

C3 A$ + 50 3 tr\A 2-° 3 8 coo L.. 7 L.

89. Answer the following questions in regards to the following three balloons - Balloon A contains helium, balloon B contains nitrogen, and balloon C contains propane - all with the same volume and at the same conditions.

b. Which one has the highest density - why?

I\J 2= 2 95/A.,e I = . 0 31,47-C. c. Which one would effuse at the fastest rate - why?

e - +Le.. I chAgAccam. viutesAx v1404_4 90. State Graham's Law and give the equation:-

I

ratIV,t6o: 4-1 -car 3a4, _A/J)

t (lV ()I'D 1964aNkxf- ̀V-1.--t_ voc4 VVIertgur- veut44,

a. Which one has the highest kinetic energy - why? - 1/4-N ,v (0)\1,

a

Name Period