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Unformatted text preview: M1MZM3 4 Peter H.Perk Marcus_ s: e
l I '
e 1 mam. Us“ 3‘1
CI[EIUHSTRY l HillSECTION 14km
Test # I
Fall lﬁ‘ilﬁ LI}. BUTTDMLEY There are 20 equal}; weighed questions on this test. Pleas: circle the correct answer for the multiple choice questions. Please
ask. lfyoude not understand The question. Please work this test Independently efynu: neighbors. notes and books. GOOD
LUCK! _ ill _ﬂ2 l 1_ _ _
l—E r—z.—ea Ema}: —h{e vDJhv (It mmmﬁx); _h_
411:
E 21 M=z=(;— l }R M=hv=ﬁ€ £4,
‘_—3 y 2 2 J' A, " v Hﬁnad lKlr'm'l'ml Pﬁv’. = Pl‘sv'2 WT: = VZJTE P'v’ = nRT MTE..GAS..A.(d§ﬁ§eﬁ] = W3
RA TE..GAS..B.[drﬁeﬂ) med um: ' g Average KE per mole = MEET 22.4 L ideal gas = 1 mole at STP Psolvent : Xselvmt Pusnlwmt ATE: = Kb m ATf = 'Kf m n=gdh nV=nRT Pl=XlP"*'l P1=fﬁ~i2 P”2
_ _ CI
Pz—kaz F's—(I'XJP 2
Avogedro's Number N, = film: at It)” m: = 9.1 x 13'“ kg
Gas Constant R. = {IﬂBZElé litm—atmfmoleK mp = 1.6? 3: III” kg
R = 3.3145 menleK ml= 1.6? x lﬂ‘ﬂkg mum I: =6.626xlﬂ‘1‘]*sec a. = 5.29:10'um  . zln'mism as 213110“! leﬂnrie=41341 lev= LE}: 10"] / usHsIou 1 PAGE 1 l. a solution contains 2.00 g of potassiu of water. What is the concentrat'
KDH [i wiwl? uroxide {as = 50.11 g mol'li in 10.00 g
of the solution exPressed in mass percent of a. 6.04% Gm]!!
h. 16.1%
c. 20.0%
d.
2. The element gallium has two naturally occurring isotopes. The Eirsr 1590a} has a relative mass of 60.925? and a fractional abundance of 0.004. and the second {TlGa} has a relative mass of 10.0209 and a fractional abundance of 0.395. Based
on these values, the chemical relative atomic mass of gallium is ‘ili 00.7
4. 69.9
c. T0.1
d. 10.3
3. Compute the relative molecular mass of Zniﬂcozjz on the 120 soale.i.e molecular
weight“ (a! 33 '
a. 123.4 *PZ" lro 1
b. 139.4 14
c. 143.4 I1J§}J 2: .25: 65 14.44 4. At 20“: the density of methanol [CH30H} is 0.?91 qiml. If a laboratory worker
needs 215 g or methanol for an experimentIr how many liters should be used? / VERSIGN 1 PAGE 2 5. Propene gas {caﬂﬁ} burns completely in an oxygen atmosphere to produce carbon dioxide and water as the only products. If the reaction is described with a
balanced chemical equation using the smallest whole number coefficients, the coetficient for water would be For the following question{sj, consider the production of ammonia gas through the
reaction of nitrogen with hydrogen as described by thenbalanced equation “2 +3H2 aims m 6. How many grams of NH3 will be produced by the complete reaction of 3.91 g of H2? 25.1 g oneIII HT
6’ 50.2 g
15.3 g
a. 1m g Hrol'
at?"
r. The followinoﬂquestionlsl concern the production of acetylene gas [Czﬂgl by the
reaction of calciumcarbide {Ceca} reacts with water as described in the balanced equation
Icacz + 2 £1204 caioH}: + can“ .9
«IIF "PH 5
xr‘bc
K t T. I How many liters of CEHZ will be produced by the complete reaction of 23.5 g of
I ‘II. ,;' Ceca Iwith. 10.0 g of water? I melt‘7 ZEN(,1.
RH::f a. 0.4451. éw'154aa‘ “aﬂfl'ifpoh: . H.555 L .531. Clﬂl—‘Eﬂ Zak mfg/o”Fr ,LfLH'” .6; * CAD Fvﬁnﬂf‘ + (£0 Vcnﬂr‘
P VERSION 1 PAGE 3 B. If 13 g of CaCz reacts to produce 0.2ﬂ0 mol of C232, the percentage yield of the
reaction would be 35%
53*
. 30% . 9M:
9 11% 9. Write the correct name or symbol in the blank space. norm s ol Name Pb lead
a 5.. I04! Magnesium
[Jam Sodium _%_ Mercury 10. Write the correct name or formula in the spaces below. Name Formula Barium nitrate Potassium permanganate I a ‘r 63,4 no;
gu.,g»‘1(::ﬂim~VL NP.th Diphorphouo pentaoxide E; gps VERSION 1 PAGE i 11. one mole of any element has a mass in grams equal to: a. avogradro's number the weight of a single atom
che atomic mass
. the atomic number
e. the atomic mass divided by avogradro's number 12. How many atoms are there in 36 grams of carbon?
a. 6.02 x 1033
o. 2.11 x 1025
.81 x 1o24
. 2.1a x 1o23
e. 1.31 x 1o23
13. Give the empirical formula of a compound which contains 52.2% carbon, 13.0%
hydrogen and 34.8% oxygen. 
(:bLJD C) “14° C' Iloq 4: “LBSMJ 1'2,
44' 1.0: e 11.27 m' s: a.
O‘Iébﬁ 4 3413‘s” ‘3' ” 14. What is the molality of a solution which contains 15.ﬂ 9 HCl in 100 g of water? 322:.” W WW d. 0.15U m
e. lSﬂ m 15. a solution contains 2.oo g of potassium hydroxide in“  55.11 g mo1”1} in 10.00 g
of water. What is the concentration of the solution expressed in mass percent of
KOH
I! win}? 1 .r M
@533: 15' ~03“ K c. 20.01: :‘Sffﬂgf M?) o 25ﬁi 12
a“! VERSION 1 PAGE 5 16. In order to prepare 0.250 L of a 0.115 M HaEr solution. a technician must mix a. 0.115 moles of NaBr with 0.250 L of H20.
b. 0.115 moles of was: with 0.250 kg of H20.
c. 0.02025 moles of NaEr and enough H20 to result in 0.250 kg or solution. c::> 0.02015 moles of East and enough H20 to result in 0.250 L of solution. mu!
mﬁr u. )02.35%.r “‘3' I. 'W .mﬁﬁm’
1?. What volume of a 15.6 H H003 solution will be needed to prepare 350 mL of 2.00 M
H1003?
II9MQ;
a. 22.2 mL h. 36.7 mL
13.4 mL
“9 m“ I
what is the percent nitrogen in in N205? o, 13%.1y/ﬂ 18
ct @ 24.1 W “3.05 N1 0; *3 * ﬁchpaf
or  7  ' 25" 9; c. 13.: We in: d :3: dz. *5 23034.! m‘ISi ' I 213913 19. Consider the reaction:
3 Cults} + 3 “03'1an =5.) 3 C11 {malgtaq} + ‘1 H20 + 2 mtg}
Iﬂqﬁlmhﬁ 6.3 grams of on reacts with 100 ml or 1.0 H nitric acid. Which of the Eollowing
statements are true. cal—ﬂarﬁﬂd—uitflctecid react in a 1:1 mole ratio.
41.4:eesche"&tmctinqﬁreactant and 0.062 moles of Hﬂoa are left over. 3 is the limiting reactant and 0.052 moles of Cu are left over. .di_ﬂueadHﬂo3*ere present in stoichiometric amountswneither in excess. e. 0.000 moles of water is produced. ’régli'lmbr "ﬁlo! ...
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 Spring '08
 Bottomley
 Atom, Atomic Mass, Atomic Number, Mass, a. avogradro

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