practice final exam #1 Flashcards by Zachary Oliver

Give the chemical formula for sulfurous acid

a. H2SO4
b. H2SO3
c. H2SO2
d. H2S
e. H2Se

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Which terms best describes the relationship between ^12C ^13C and ^14C ?

a. isomers
b. isotopes
c. allotropes
d. diatomics
e. triatomics

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What mass of carbon is present is 1.5 x 10^22 molecules of C4H10O2 ?

a. 0.12g
b. 1.2g
c. 0.3g
d. 0.6g
e. 3.0g

b. 1.2g

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Which of the following is the balanced chemical reaction for the combustion of C2H6O ?
It’s not letting me copy/paste so just figure it out, please

C2H6O + 3O2 = 2CO2 + 3H2O

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What is the mass percentage of nitrogen in N2O4 ?

a. 15%
b. 30%
c. 40%
d. 55%
e. 70%

30%

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If eleven moles of P and twenty moles of Cl2 react completely, what is the reagent in excess and how much remains after completion?
2P + 5Cl2 = 2PCl5

a. P, 3 moles
b. P, 6 moles
c. P, 9 moles
d. Cl2, 6 moles
e. Cl2, 9 moles

P, 3 moles

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What volume of 4M NaOH is required to produce 800 ml of 0.25M NaOH?

a. 12.5 ml
b. 25 ml
c. 50 ml
d. 100 ml
e. 200 ml

50 ml
(C1)(V1) = (C2)(V2)

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A 20 gram sample of a metal was heated to 100 degrees C and then added to 20 grams of water at 10 degrees C. What is the specific heat of the metal? cwater = 4.184 J/gK

a. 0.26 J/gK
b. 0.52 J/gK
c. 0.78 J/gK
d. 1.2 J/gK
e. 33.5 J/gK

0.52
(cmetal)(-80C) = -(4.184)(10C)

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How much heat would be required to heat 108 grams of solid aluminum at 2419 degree C to liquid aluminum at 2519 degrees C?
aluminum melting point: 2519 degrees C
cAl = 0.90 J/gK
deltaH fusion = 660 kJ/mol

a. 39,000 kJ
b. 39 kJ
c. 2.6 kJ
d. 2650 kJ
e. 12,640 kJ

2650 kJ
q = mcdeltaT

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What is the ground state electron configuration of Ni^2+ ?

a. I’m not writing out all this shit
b.
c.
d.
e.

1s^2 2s^2 2p^6 3s^2 3p^6 3d^8

Idk. I guess there are 2 less electrons than normal and I know they’re removed differently than they’re added

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What is the maximum number of electrons that can occupy a d orbital?

a. 1
b. 2
c. 5
d. 10
e. none of these

2
kind of a trick question. the orbital is just the box and only 2 electrons can occupy one box no matter what shell it’s in

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Which of the following groups has a valence shell electron configuration of ns^2 np^5 ?

a. alkali metals
b. alkaline earth metals
c. chalcogens
d. halogens
e. noble gases

d. halogens
7 valence electrons
I just used fluorine as an example and yeah, 2p^5

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Which of the following has the shortest bond length?

a. C-O
b. Si-O
c. C-F
d. C-Cl
e. C-Br

C-F
smaller atoms, smaller bond length

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Which of the following has the highest (most negative) electron affinity?

a. Si
b. P
c. S
d. Cl
e. Ar

Cl
Cl has a higher affinity than F also so… Just remember that

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Which of the following has both ionic and covalent bonds?

a. N2
b. NaCl
c. KOH
d. H2O
e. HCl

KOH

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Which of the following is the correct Lewis dot structure for O3?
Just draw it.
hint: it’s assymetrical

…

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The bond formed between 2 elements with high electron affinities in likely to be…

a. ionic
b. covalent
c. metallic
d. coordinate covalent
e. cannot be determined

covalent

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Which of the following is the best Lewis dot structure for HSO3-
Just try to draw it.
hint: the H atom isn’t where it would seem based on how it’s written

…

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Arrange the following in order of increasing carbon-carbon bond length.
hint: benzene has a length between a single and a double bond
I. benzene II. HC triple bond CH
III. H2C double bond CH2 IV. H3C single bond CH3

a. II I III IV
b. II III IV I
c. II III I IV
d. IV I III II
e. I IV III II

c.
a triple bond is shorter and stronger than a double bond which is shorter and stronger than a single bond

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What is the hybridization of Cl in ClF5?
refer to study guide

a. sp
b. sp2
c. sp3
d. dsp3
e. d2sp3

d2sp3
1 non bonding pair and 5 bonding

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What are the approximate bond angles around the central atom in AsCl3?
hint: refer to study guide (I have no interest in memorizing all this shit)

a. 90 degrees
b. 109.5 degrees
c. 120 degrees
d. 90 and 120 degrees
e. 90 and 180 degrees

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109.5 degrees

Which of the following has a molecular geometry that is trigonal planar?
hint: refer to study guide (I have no interest in memorizing all this shit)

a. AsH3
b. SiCl4
c. CH2O
d. SF6
e. SO2

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CH2O

What is the molecular geometry of PF6-?
hint: refer to study guide (I have no interest in memorizing all this shit)

a. octahedral
b. square pyramidal
c. t-shaped
d. see-saw
e. trigonal bipyramidal

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a. octahedral

What the the volume of 64 grams of oxygen gas at a pressure of 600 torr and a temperature of 12 degrees C ? (assume ideal behavior; R = 0.0821 L(atm)/mol(K)

a. (4)(0.0821)(285) / 600
b. (4)(0.0821)(285)(760) / 600
c. (4)(0.0821)(285)(600) / 760
d. (4)(0.0821)(12)(760) / 600
e. (2)(0.0821)(285)(765) / 600

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Which of the following is true about equal volumes of Ne and Ar at STP? a. Ar has twice the kinetic energy as Ne b. the sample of Ne has twice the rms velocity as the sample of Ar c. the sample of Ar has twice the density of Ne d. both samples have the same rms velocity e. the sample of Ar has twice the pressure of the sample of Ne

the sample of Ar has twice the density as the sample of Ne

What is the pressure of the gas trapped in the mercury nanometer? So the gas is on the left and the liquid is 40 cm higher on the right a. 340 mm Hg b. 400 mm Hg c. 800 mm Hg d. 1160 mm Hg

1160 mm Hg

Which of the following compounds has the highest heat of vaporization? hint: which has the highest attractive forces a. BH3 b. CH4 c. SiH4 d. PH3 e. AsH3

AsH3

Which of the following affects the vapor pressure of liquid? I. surface area II. temperature III. pressure a. II only b. III only c. II and III d. I and III e. I, II, and III

temperature only

Which step in the reaction diagrammed below has the largest rate constant? hint: draw it so it's a graph with 'reaction coordinate' as the x-axis and 'energy' for the y-axis. the curve shoots up and makes 3 camel humps on its way back down. the first hump being the highest. the second; the next highest. and the third hump being the shortest. hint: the step with the highest rate constant will be the fastest step a. 1st step b. 2nd step c. 3rd step d. 4th step e. cannot be determined

For the reaction A + B = C the following kinetic data was obtained: A B Initial Rate (Ms^-1) 0.026 0.017 0.050 0.052 0.017 0.20 0.052 0.051 0.60 What is the overall reaction order? a. 0 b. 1 c. 2 d. 3 e. 6

Which of the following if false concerning a catalyst? a. a catalyst is not consumed in the reaction b. a catalyst lowers the activation energy of a reaction c. a catalyst shifts the equilibrium toward the products and increases the yield d. a catalyst lowers the activation energy of the reverse reaction e. a catalyst provides an alternatae pathway for the reaction to occur

What is the correct equilibrium constant (Kc) expression for the following reaction? 4Fe(s) + 4O2(g) = 2Fe2O3(s) hint: solids basically don't count a. Kc = [Fe2O3] / [Fe][O2] b. Kc= [Fe2O3]^2 / [Fe]^4 [O2]^3 c. Kc= 1 / [O2}^3 d. Kc= [Fe][O2] / [Fe2O3] e. Kc= [Fe]^4 [O2]^3 / [Fe2O3]^2

Consider the following reaction at equilibrium: 2CO(g) + O2(g) = 2CO2(g) deltaH = -566 kJ Which of the following would increase the amount of CO2 present? a. removal of CO b. the addition of a catalyst c. raising the temperature d. an increase in the pressure e. none of these

an increase in the pressure

Which of the following must be true about a reversible reaction that has reached equilibrium? a. the reaction has stopped completely in both directions b. the forward rate constant equals the reverse rate constant c. Kc = 1 d. the concentration of reactants and products are not changing e. the concentration of reactants equals the concentration of products

What is the pH of 0.01 M HOCl (Ka = 3.5 x 10^-8)? hint: [H^+] = the square root of Ka[Ha] a. 2.0 b. 3.8 c. 4.7 d. 7.0 e. 9.3

4.7

Which of the following is true about the titration of 0.1M acetic acid (HC2H3O2, Ka = 1.8 x 10^-5) with 0.1M NaOH a. at the equivalence point pH = 7, at the half equivalence point pH = 3.5 b. at the equivalence point pH > 7, at the half equivalence point pH = 4.8 c. at the equivalence point pH < 7, at the half equivalence point pH = 4.8 d. at the equivalence point pH > 7, at the half equivalence point pH = 3.5 e. at the equivalence point pH = 7, at the half equivalence point pH = 4.8

A 0.010M solution of an electrolyte has a pH of 10.2 Which of the following best describes this electrolyte? a. weak acid b. weak base c. strong acid d. strong base e. non-electrolyte

weak base

Which of the following, when dissolved in water, will have a pH greater than 7? a. HNO3 b. CsNO2 c. Al(NO3)3 d. NaNO3 e. RbCl

CsNO2

What is the correct Ksp expression for La(IO3)3? a. Ksp = [La^3+][3IO3-]^3 b. Ksp = [La^3+][IO3-]^3 c. Ksp = [La^3+][3IO-]^3 d. Ksp = [La^3+][IO-]^3 e. Ksp = [La^3+]3[IO3-]^3

The molar solubility of Ag2CO3 is 1.3 x 10^-4 M. What is its Ksp? a. 2.2 x 10^-12 b. 1.7 x 10^-8 c. 1.1 x 10^-2 d. 8.8 x 10^-12 e. 2.9 x 10^-16

Calculate deltaH for the following reaction: CH4(g) + 2O2(g) = CO2(g) + 2H2O(g) Bond Enthalpies kJ/mol C-H 413 C-O 358 C double bond O 799 O-O 146 O double bond O 495 O-H 463 a. -1214 kJ b. -808 kJ c. -354 kJ d. +354 kJ e. +1214 kJ

For which of the following reactions is deltaHrxn = deltaHf ? a. NO(g) + 1/2O2(g) = NO2(g) b. C(diamond) + 1/2O2(g) = CO2(g) c. CaO(s) + H2O(l) = Ca(OH)2(s) d. Ca(OH)2(s) = CaO(s) + H2O(l) e. 2C(graphite) + O2(g) + 2H2 (g) = CH3COOH(l)

Given the following deltaH values C2H2(g) + 2H2(g) = C2H6(g) deltaH = -311 kJ 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(l) deltaH = -3120 kJ H2(g) + 1/2O2(g) = H2O(l) deltaH = -286 kJ What is the deltaH for the following reaction? C2H2(g) + 5/2 O2(g) = 2CO2(g) + H2O(l) a. -3717 kJ b. -2443 kJ c. -1871 kJ d. -1299 kJ e. 2809 kJ

Which of the following statements is correct concerning the following reaction: N2O4(g) = 2NO2(g) deltaH = 58 kJ a. the reaction is spontaneous at all temperatures b. the reaction is non spontaneous at all temperatures c. the reverse reaction is spontaneous at all temperatures d. the reaction is only spontaneous above a certain threshold temperature e. the reaction is only spontaneous below a certain threshold temperature

What is the oxidation state of phosphorus in H3PO2? a. -3 b. -1 c. +1 d. +3 e. +5

What is the oxidizing agent in the followng reaction? Pb(s) + PbO2(s) + 2SO4^2-(aq) + 4H^+(aq) = 2PbSO4(s) + 2H2O(l) a. Pb b. PbO2 c. SO4^2- d. H^+ e. PbSO4

Which of the following is false regarding a galvanic cell? a. Ecell is positive b. Electrons travel through the salt bridge from anode to cathode c. deltaG is negative d. The anode is negative e. The reaction is spontaneous

What is the Ecell for the following reaction? 3Ni + 2Al^3+ = 3Ni^2+ + 2Al And then there's a whole table of reduction potentials. I would just ask Chat to generate all the info that you would need to solve this problem on a table because I really don't want to copy it all and it's not letting me copy/paste a. -2.57V b. -1.91V c. -1.41V d. 1.41V e. 1.91V

-1.41V

How many moles of zinc are produced if the molten electrolysis of ZnCl2 is performed with a current of 50 Amps for 40 minutes? (use F = 96,500 C/mol e^- a. (50)(40)(65.4) / (2)(96500) b. (50)(2400)(18.4) / (2)(96500) c. (50)(2400)(65.4) / (2)(96500) d. (50)(2400) / (2)(96500) e. (50)(40) / (2)(96500)

A radioactive nuclide has a half-life of 17 years. How much of an 80 gram sample would remain after 100 years? honestly: you can work this out with a calculator and some logic. hint: the answer doesn't work out perfectly in 17 year intervals a. 0.8g b. 1.7g c. 2.8g d. 17g e. 20g

1.7g

practice final exam #1 Flashcards

(51 cards)