practice final exam #2 Flashcards by Zachary Oliver

Give the chemical formula of potassium permanganate
hint: MnO4 has a -1 charge

a. K3MnO4
b. K2MnO4
c. KMnO4
d. K2MnO3
e. KMnO3

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The relative abundances of an element in a parallel universe are 85% ^20X and 15% ^22X. Which of the following is the best approximation of the atomic mass for element x?
hint: the equation is pretty easy. it’s more of a sum problem than an average problem.

a. 20
b. 20.3
c. 20.9
d. 21.2
e. 21.7

20.3

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What is the IUPAC name for NO?

a. mononitrogen monoxide
b. mononitrogen oxide
c. nitrogen (III) oxide
d. nitrogen monoxide
e. nitrogen (II) oxide

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What is the mass percent of fluorine in rubidium fluoride?

a. 18%
b. 35%
c. 50%
d. 61%
e. 82%

18%

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How many atoms are present in a 6 gram sample of NaCl?
I hate this fraction answer shit because I don’t do this exactly the same. I would just solve the problem and then do the mulitiplication for each answer.

a. (6)(6.02 x 10^23)(2) / (58.4)
b. (6)(58.4) / (6.02 x 10^23)
c. (6)(6.02 x 10^23) / (58.4)
d. (6)(58.4)(2) / (6.02 x 10^23)
e. (6) / (58.4)

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What is the maximum mass of Fe2O3 that could be produced from 9.0 grams of FeO and excess O2?
4FeO + O2 = 2Fe2O3 ?

a. 0.125g
b. 1.25g
c. 4g
d. 10g
e. 100g

10g

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3.0 x 10^21 molecules of a substance weights 0.10 grams. Which of the following could be this substance?

a. Ar
b. LiH
c. CH4
d. HF
e. none of these

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How much heat would be required to raise the temperature of 30 grams of ice from a temperature of -73 C to -18 C (cice = 2.05 J/gK

a. (30)(2.05)(328)
b. (30)(55) / (2.05)
c. (30)(2.05)(55)
d. (30)(2.05) / (55)
e. (30)(328) / (2.05)

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What is the ground state electron configuration of Fe^2+ ?
I’m not writing all this shit. Just write it and compare with the answer.
hint: when removing electrons, remove from the highest shell first e.g. the 4 shell

1s2 2s2 2p6 3s2 3p6 3d6

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Which of the following has the greatest number of valence electrons?
just look at the p-table

a. Ga
b. Cr
c. C
d. Ti
e. Rb

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Which of the answer choices has an electron configuration of [Ar] 4s2 3d3?

a. Ti
b. Cr^2+
c. Mn^2+
d. V
e. Fe^3+

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Which of the following has the largest radius?

a. Be
b. Mg
c. Ca
d. Sr
e. Sr^2+

Sr
I think with Sr^2+ it has lost electrons and so there is more pull from the positive nucleus which would make it smaller

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Which of the following has the highest 1st ionization energy?
hint: ionization energy is the energy needed to remove an electron

a. Be
b. Ca
c. Cs
d. C
e. Rb

C
all the others ‘want’ to lose electrons

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Which of the following would be expected to behave chemically most similar to strontium?

a. Ar
b. Cl
c. Cs
d. Mg
e. Mn

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Which of the following is the correct Lewis dot structure for ClO3- ?
refer to study guide for rules form Lewis dots

honestly, just look it up online and compare
2 of the oxygens have double bonds and there’s a lone pair on Cl

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Which of the following structures has an atom(s) that violate(s) the octet rule?
I. BH3 II. SCl2 III. N2O

a. I
b. II
c. I and II
d. I, II, and III

I. only
it is very common for B to violate the octet rule

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Which of the following has the most polar bond?

a. H-F
b. H-Cl
c. C-Br
d. H-Br
e. H-I

a. H-F
It’s all about the greatest difference in electronegativity. F has the highest electronegativity since electronegativity trends up and to the right.
Electronegativity is a measure of an atom’s ability to attract shared electrons towards itself when it’s in a chemical bond

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What is the hybridization of Br in BrF4- ?
hint: just refer to study guide

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

d2sp3

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What is the molecular geometry of BrF5 ?
hint: refer to study guide

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

square pyramidal

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What is the molecular geometry of SeF4 ?
hint: refer to study guide

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

d. see-saw

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If the volume of gas behaving ideally is 1.5L at a pressure of 300mmHg and a temp of 30 degrees C, what will it’s volume be at a pressure of 100mmHg and a temp of 15 degrees C ?

a. 0.3L
b. 2.8L
c. 4.3L
d. 9.0L
e. 12L

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4.3L

P1V1 / n1T1 = P2V2 / n2T2

If an equal number of moles of N2, O2, Ar, and Ne are introduced into a balloon having a tiny leak, which of the following is true about the respective partial pressures of the gases in the balloon after 30 minutes?
hint: you don’t need the equation because they’re all equal number of moles. However, don’t forget the diatomics will have twice the weight of just their single atom

a. pN2 > pO2 > pAr > pNe
b. pAr > pO2 > pN2 > pNe
c. pAr > pNe > pN2 > pO2
d. pAr > pN2 > pO2 > pNe
e. pO2 > pN2 > pAr > pNe

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b.
So basically the lighter gases escape first leaving more of the heavier gases present

Which of the following has the highest boiling point?
hint: greatest intermolecular foreces will have the highest boiling point

a. F2
b. Cl2
c. Br2
d. I2
e. He

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I2
I think the only IMF’s at play here are London-dispersion which increase with greater molecular weight and surface area (not always the same thing)
So iodine is clearly the fattest of these

Which of the following compounds has the highest vapor pressure?
hint: highest vapor pressure = lowest attractive forves. Like: there’s less holding them together so they start floating up in the air

a. H2O
b. H2S
c. H2Se
d. H2Te
e. C6H12O6

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H2S

H2O and C6H12O6 have hydrogen bonding so those are pretty strong
H2S (and this is what I don’t really get) is the most polar of the rest of the choices but has the smallest surface area (least London-dispersion forces) so that makes it have the lowest intermolecular forces overall
So I though LD forces were weak but also polar forces really don’t seem to count for shit

Which of the following could be the triple point for water? just being real: I don't have a good grasp on this triple point shit at all a. -1.0C / 0.0060 atm b. 101C / 60 atm c. 0.01C / 0.0060 atm d. 99C / 6.0 atm e. 0.01C / 1.01 atm

If the vapor pressure of pure benzene and pure hexane at a certain temperature are 240 torr and 300 torr respectively, then what would be the vapor pressure of benzene at this temperature above a solution with a 19:1 benzene to hexane ratio? a. 120 torr b. 228 torr c. 252 torr d. 285 torr e. 528 torr

228 torr pbenzene = xbenzene P*benzene where x is the mole fraction (literally a fraction) and P*benzene is the vapor pressure of pure benzene pbenzene = (19/20)((240torr) = 228 torr

Which of the following from the diagram represents the activation energy of the reverse reaction? basically you have a flat line on the left which starts sloping up to make a hump, the hump heads back down again until it ends in another flat line on the right that's below the original flat line. So draw that and then draw a vertical line where the activation energy would be reprsented for the reverse reaction

the line should go from the flat line on the right (the lower one of the two) all the way up to the hump

Doubling the concentrations of both reactants in the following reaction increases the rate of reaction by a factor of 4. A + 2B = C Which of the following could be the rate law? a. rate = k[A][B]^2 b. rate = k[A]^2[B]^2 c. rate = k[A]^2[B] d. rate = k[A]^2 e. rate = k[B]

d. if doubling the concentration of both reactants results in an increase in the rate by a factor of 4, then the reaction must either be 2nd order in one reactant and zero order in the other

If the average rate of disappearance of O2(g) in the following reaction is 0.010 atm/s, then what is the average rate of disappearance of C2H6(g) in the following reaction? 2C2H6(g) + 5O2(g) = 4CO2(g) + 6H2O(l) a. -0.025 atm/s b. 0.025 atm/s c. 0.4 atm/s d. 0.04 atm/s e. 0.004 atm/s

e. 0.004 atm/s

For the reaction A2 + B = AB + A, the following kinetic data were obtained: A2 at zero M B at zero M Initial rate Ms^-1 0.014 0.015 0.050 0.014 0.015 0.050 0.028 0.030 0.10 What is the rate law? a. rate = k[A2][B]^2 b. rate = k[A]^2[B] c. rate = k[A2] d. rate = k[B] e. rate = k[A2]^2[B]^2

If 3 moles of both H2 and Cl2 are introduced into a 1.5L vessel, what will be the equilibrium concentration of HCl in the vessel? H2(g) + Cl2(g) = 2HCl(g) Kc = 16 a. 0.33 M b. 0.67 M c. 1.33 M d. 2.67 M e. 4.0 M

Given the following: N2(g) + 1/2O2(g) = N2O(g) Kc = 1.0 x 10^-18 What is the equilibrium constant of the following reaction? 2N2O = 2N2(g) + O2(g) Kc = ? a. 2.0 x 10^-18 b. 2.0 x 10^18 c. -2.0 x 10^-18 d. -2.0 x 10^18 e. 1.0 x 10^36

Which of the following is false regarding an equilibrium constant? a. Kc = kf / kr b. lowering the activiation energy does not change the value of the equilibrium constant c. increasing the concentrations of the products increases the value of the equilibrium constant d. a change in pressure will not change the equilibrium constant

Under which of the following conditions would the amount of CO2 produced be maximized? 2CO(g) + O2(g) = 2CO2(g) deltaH = -566 kJ a. high temps and high pressures b. high temps and low pressures c. low temps and high pressures d. low temps and low pressures e. low temps at constant pressure

How much greater is the concentration of [H^+] at pH 8 than at pH 9.5? a. 1.5 times greater b. 15 times greater c. 32 times greater d. 105 times greater e. 300 times greater

What is the pH of 0.10M KCN? (Ka, HCN = 4.9 x 10^-10) (check the formulas on the study guide for questions like this) a. 2.9 b. 3.1 c. 8.9 d. 10.9 e. 11.1

Which of the following solutions would have the highest pH? a. 0.01M HCL b. 0.01M NaF c. pure H2O d. 0.01M KOH e. 0.01M NH3

What is the pH of a solution containing 0.2M HOCl (Ka = 3.0 x 10^-8) and 0.6M NaOCl? a. 6.0 b. 6.5 c. 7.0 d. 7.5 e. 8.0

What is the concentration of F- in a saturated solution of PbF2? Ksp, PbF2 = 4.0 x 10^-8 a. 2.2 x 10^-3M b. 4.4 x 10^-3M c. 4.8 x 10^-6M d. 1.9 x 10^-5M e. 2.0 x 10^-4M

What is the molar solubility of ZnC2O4? Ksp, ZnC2O4 = 2.7 x 10^-8 a. 3.0 x 10^-3M b. 1.9 x 10^-3M c. 1.3 x 10^-2M d. 3.1 x 10^-2M e. 1.6 x 10^-4M

Based on the following, what is the enthalpy of formation of N2O(g)? 2N2O(g) = 2N2(g) + O2(g) deltaH rxn = -163.2 kJ a. -326.4 kJ b. -163.2 kJ c. 81.6 kJ d. 163.2 kJ e. 326.4 kJ

For what type of reaction would it be expected that the deltaG would be largely independent of a change in temperature? a. endothermic b. exothermic c. deltaH ~ zero d. deltaS ~ zero e. deltaG < zero

deltaS ~ zero

Which of the following phase changes is endothermic? I. fusion II. condensation III. deposition a. I only b. I and II c. II and III d. III only e. I, II, and III

Use the provided enthalplies of formation to calculate deltaH for the following reaction? Na2CO3(s) + 2HCl(aq) = 2NaCl(aq) + H2O(l) + CO2(g) deltaH fusion kJ/mole Na2CO3(s) -1131 HCl(aq) -137 NaCl(aq) -407 H2O(l) -286 CO2(g) -394 a. -2959 kJ b. -211 kJ c. -29 kJ d. 29 kJ e. 211 kJ

What is the oxidation state of iron in Fe3O4? find oxidation rules a. 0 b. +1 c. +2 d. +3 e. none of these

e. It really is 8/3 (according to the test). It's the first time I've ever seen mention of a fractional oxidation state.

According to the table of reduction potentials, which of the following is the strongest reducing agent? Table of reduction potentials: Al^3+ + 3e^- = Al -1.66V Mn^2+ + 2e^- = Mn -1.18V Zn^2+ + 2e^- = Zn -0.76V Cr^3+ + 3e^- = Cr -0.74V Fe^2+ + 2e^- = Fe -0.44V Co^2+ + 2e^- = Co -0.28V Ni^2+ + 2e^- = Ni -0.25V 2H^+ + 2e^- = H2 0.00V Cu^2+ + 2e^- = Cu +0.34V Ag^+ + e^- = Ag +0.80V a. Al^3+ b. Ag c. Ag^+ d. Ni e. Cu

What is produced at the anode in the molten electrolysis of CaO? a. Ca b. Ca^2+ c. O^2- d. O2 e. H2O

How many moles of electrons would be required to make 2.4 grams of titanium in the molten electrolysis of TiCl4? a. 0.05 b. 0.1 c. 0.2 d. 0.4 e. 2

A radioactive nuclide has a half-life of 12 minutes. How long will it take until only 12.5% of the sample remains? a. 4 minutes b. 6 minutes c. 24 minutes d. 36 minutes e. 48 minutes

Which of the following will result in a change in the mass number of the parent nucleus? a. positron emission b. beta decay c. alpha decay d. electron capture e. gamma emission

alpha decay

practice final exam #2 Flashcards

(51 cards)