Chemical Processes Flashcards

1
Q
Which molecule is nonpolar?
A. carbon monoxide
B. acetone
C. carbon tetrachloride
D. ethanol
A

C. Carbon tetrachloride is the only nonpolar compound because it is the only compound listed in which all of the electrons are shared equally across the four same bonds; each chlorine atom bonds with the carbon atom with the same force. Consequently, carbon tetrachloride exhibits a tetrahedral structure with geometric symmetry

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2
Q
A 50ml solution of HCl is diluted to 250ml at 10M. What was the initial concentration of the HCl?
A. 500M
B. 50M
C. 5M
D. 0.5M
A

B. The product of the initial concentration and the initial volume is equal to the product of the final concentration and the final volume of the solution. This can be remembered as c1v1=c2v2
Substitute the known quantities and solved for the unknown: c1:c150ml=10M250ml —-> c1=50M

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3
Q
What product results from treating ethanol with pyridinium chlorochromate (PCC)?
A. acetaldehyde
B. formaldehyde
C. acetone
D. acetic acid
A

A. PCC is a mild oxidizing reagent used to oxidize primary alcohols to aldehydes. Ethanol, a primary alcohol, treated with PCC results in a 2 carbon aldehyde called ethanal or acetaldehyde

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4
Q
What are the relative pKa values of the following compounds? I. H2O, II. NH3, III. HCl, IV. CH3COOH
A. II > I > IV > III
B. IV > II > III > I
C. III > IV > I > II
D. I > III > IV > II
A
A. Categorize the options as strong acids, weak acids, neutral, weak bases, or strong bases and rank. Low pKa values correspond to higher acidity levels
Carboxylic acids= 4-5 pKa
Water= 15.7 pKa
Amines= 36 pKa
Alcohols= 15-18 pKa
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5
Q
What is the oxidation number of nitrogen in NF3?
A. -3
B. 0
C. +2
D. +3
A

D. The sum of the oxidation numbers of a neutral compound is always 0. The oxidation number of fluorine is always -1. Let x represent the oxidation number of N, set up the equation, and solve for x: x + (-1) *3=0 —> x=3

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6
Q
What is the conjugate base of sulfuric acid?
A. H2SO3
B. HSO4-
C. SO4 -2
D. H3SO4+
A

B. In a solution, sulfuric acid will donate an H+ to water to form hydronium H3O+. The loss of the single H+ results in H2SO4 becoming HSO4-

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7
Q

What would be the result of increasing the number of nucleophiles in a Sn1 reaction?
A. it would increase the rate exponentially
B. it would increase the rate linearly
C. it would decrease the rate
D. it would have no effect

A

D. Sn1 reaction are substitution reactions that depend on reagents attracted to electrons (electrophiles). Sn1 reactions do not depend on the number of nucleophiles involved in the reaction. Consequently, altering the concentration of nucleophiles does not alter the rate of reaction

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8
Q
Which of the following species cannot hydrogen bond with itself?
A. ethanol
B. acetic acid
C. ammonia
D. acetone
A

D. Hydrogen bonds occur between hydrogen of one molecule with an electronegative atom (oxygen, nitrogen, or fluorine) of another atom. Consequently, acetone is unable to hydrogen bond with itself. The hydrogen atoms in acetone are covalently bonded to carbon atoms and not a strong electronegative atom like nitrogen, oxygen, or fluorine

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9
Q
Which effect would result from increasing the molar mass of a gas?
A. an increase in temperature
B. an increase on pressure
C. an increase in volume
D. a decrease in the rate
A

D. Graham’s Law of Diffusion states that the rate of diffusion is inversely proportional to the molecular weight of the molecule. Let the initial molar mass be 5, and the increased molar mass be 10, substitute these values into Graham’s equation and compare the results

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10
Q
Rank the following amino acids by increasing pl (isoelectric point): I. Lys, II. Leu, III. Asp
A. I < II < III
B. III < II < I
C. II < I < III
D. III < I < II
A

B. The pl of a molecule is its isoelectric point, or the point at which, in this case, the amino acid will have no overall charge. Categorizing the amino acids: I is positively charge and basic; II is nonpolar and neutral; III is polar and acidic. Acidic amino acids on average have the lowest pl, nonpolar amino acids have a higher pl, and basic amino acids carry the largest pl

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11
Q
What is the result of adding HBr and hydrogen peroxide to propene?
A. 2-propanol
B. 1-propanol
C. 2-bromopropane
D. 1-bromopropane
A

D. In the presence of an organic peroxide, the addition of HBr and peroxide to a propene results in an anti-Markovnikov product in which the hydrogen becomes attached to the carbon with fewer hydrogens connected to it. The product of the addition is CH3CH2CH2Br or 1-bromopropane

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12
Q
Which of the following has the highest boiling point?
A. methanol
B. n-propanol
C. isopropanol
D. ethanol
A

B. Boiling points primarily depend upon the cohesive forces between molecules. When dealing with molecules of relatively similar molecular weights, the boiling points will depend upon the functional groups involved, and as the molecular weight of the molecule increases, the boiling point also increases. Lastly, branching decreases boiling point. With these considerations, n-propanol will exhibit the highest boiling point of the options

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13
Q

The rate law for a reaction is of the second order. Which statement is true?
A. the rate must depend on both reactants
B. the reaction must depend on the square of one reactant
C. the reaction must depend on only k squared
D. the reaction must depend on at least one of the reactants

A

D. In a second-order reaction the reaction rate is dependent upon either the product of the reactants, or the square of one of the reactants

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14
Q

The solubility of KCl in seawater would be ____ than the solubility of KCl in tap water.
A. higher
B. the same as
C. lower
D. KCl would completely insoluble in sea water as K cannot dissociate in water

A

C. Potassium chloride is a metal halide salt. While it dissolves readily in water, its solubility is lowered because of the common ions present in the seawater. This is otherwise known as the common ion effect

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15
Q
An electron pair donor is best classifies as a:
A. strong acid
B. Bronsted-Lowry acid
C. Lewis acid
D. Lewis base
A

D. By definition, a Lewis base is an electron pair donor. A Lewis acid, on the other hand, is an electron pair acceptor

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16
Q
Which reaction can be spontaneous under favorable conditions? I. -TH, +TS  II. -TH, -TS   III. +TH, -TS
A. I only
B. II only
C. I and III only
D. I and II only
A

D. Under favorable conditions, TH < 0, and TS > 0, a reaction will be spontaneous at any temperature. If one of the conditions is unfavorable with either TH > 0 or TS <0, a reaction can be spontaneous if it satisfies TG < 0 using the standard-state free energy of reaction equation: TG=TH-TTS. Roman numeral III can never be spontaneous

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17
Q
Which of the following alcohols is the most easily dehydrated?
A. (CH3)3C-OH
B. (CH3)2CH-OH
C. CH3CH2-OH
D. CH3-OH
A

A. Classify the alcohols as primary, secondary, or tertiary: A is tertiary because the -OH group is directly attached to the 3 alkyl groups; B is secondary because the carbon attached to the -OH is connected to two carbon atoms; C is primary because the carbon connected to the -OH group is connected to one carbon atom; and although D lacks an attached alkyl group, it is considered primary.. As tertiary alcohols form the most stable carbocations, A is correct

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18
Q
If the pl of a specific protein is 6, what is the charge on the protein when it is in a solution of pH 9?
A. -
B. 0
C. +
D. cannot be determined
A

A. The pl, or the isoelectric point, is the pH at which a molecule exhibits a net charge of 0. When the pl of a molecule is less than the pH of the surrounding solution, the molecule is deprotonated and its charge is negative. The 3 situations:
pH < pl = protonated +
pH > pl = deprotonated -
pH = pl = neutral charge

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19
Q
What is the hybridization of the carbons in benzene?
A. s
B. sp
C. sp2
D. sp3
A

C. Benzene, C6H6, is a plana regular hexagon made up of a ring of carbon atoms. Each carbon is bonded with 2 other carbon atoms as well as a hydrogen atom fro a total of 3 bonded atoms. Consequently, the hybridization of benzene is sp2

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20
Q
What is the conjugate acid of HCl?
A. Cl-
B. Cl2-
C. H2Cl+
D. H2O
A

C. The conjugate acid of a compound results from the addition of a proton H+. The theoretical conjugate acid of HCl would be: HCl + H+ —-> H2Cl+

21
Q
Which of the following are reducing agents?
A. FADH2
B. NAD+
C. NADH
D. Both A and C
A

D. Reducing agents are those that donate electrons in redox chemical reactions. Cellular respiration involves the carrying of electrons by both FADH2 and NADH. Because both must be included in the answer, D is correct

22
Q
What is the partial pressure of nitrogen in a gas of 30 atm made of equal moles of oxygen, nitrogen and carbon?
A. 3 atm
B. 10 atm
C. 15 atm
D. 30 atm
A

B. Dalton’s Law states that the total pressure of a gas mixture is equal to the sum of the partial pressures. In this case, the total pressure is 30 atm, which is the result of 3 equally combined gases.

23
Q
Which effect does removing a solute have?
A. increases the boiling point
B. increases the melting point
C. increases the freezing point
D. decreases the vapor pressure
A

C. The addition of a solute to a solvent lowers the freezing point of the solution due to the pressure added to the solvent. Consequently, the removal of a solute from a solvent must have the opposite effect and increase the freezing point

24
Q
An element whose atomic number is 16 would have how many unpaired electrons?
A. 0
B. 1
C. 2
D. 4
A

C. The atomic number indicated the number of protons (and electrons). Writing the electron configuration: 1s2,2s2,2p6,3s2,3p4 (2+2+6+2+4=16). The 3p orbital will contain 1 filled orbital, and 2 half-filled orbitals, which indicated 2 unpaired electrons.

25
Q
If a substance has a constant half life of 10 weeks, how many grams of a 12g sample would remain after 30 weeks?
A. 8g
B. 6g
C. 3g
D. less than 2g
A

D. Thirty weeks corresponds to 3 half lives. After the first half life (10 weeks), there will be 12/2=6g after 10 weeks, 6/2=3g after 20 weeks, 3/2=less than 2g after 30 weeks

26
Q
Rank the following compounds based on increasing acidity: I. CH3HC2OH, II. CH3COCH3, III. CH3CH2COH, IV. CH3CH2COOH
A. II, III, IV, I
B. II, IV, I, III
C. II, III, I, IV
D. IV, I, III, II
A

C. There is no strong acids present in the answer choices. There is only one weak acid present in the answer choices: CH3CH2COOH. The presence of the carboxyl group indicates a weak acid. Because there are no other weak acids, IV must be the most acidic compound included

27
Q
Which of the following would show the greatest number of peaks at different values on a proton NMR?
A. CH4
B. CH3CH3
C. CH3CH2CH2CH3
D. CH3CH2CH2OH
A

D. The peaks in a proton NMR correspond to the number of different environments containing hydrogen. All the protons in methyl CH3 and methylene CH2 groups are eequivalent because they exist in the same environment. So, methyl and methylene both contain 2 peaks. 1-propanol, however, includes 3 environments CH2, CH3, OH and would contain the greatest number of peaks

28
Q
The distribution of electrons evenly in a molecule contributes to stability. This accounts for:
A. atomic mass
B. valence
C. resonance
D. electronegativity
A

C. Resonance describes the possible positions of electrons within a molecule when more than one possibility exists. Molecules that have multiple resonance structures display greater stability than those with fewer resonance structures

29
Q
Which of the following would have the highest pH in a solution?
A. hydrofluoric acid
B. water
C. ammonia
D. hydrochloric acid
A

C. Because ammonia can accept protons from water molecules, it is considered basic. Water is considered neutral, and both hydrofluoric and hydrochloric acid have low pH’s because they ionize in aqueous solutions. Ammonia, a base, has the highest pH of the answer choices

30
Q
The addition of HBr with peroxide and an alkene yields what product?
A. Markovnikov's product
B. anti-Markovnikov's product
C. Sayteffs product
D. the ortho product
A

B. In the absence of peroxide, HBr plus an alkene yields Markovnikov’s product. But, in the presence of peroxide, the result of the reaction is an anti-Markovnikov’s product

31
Q
In which locations does this reaction occur? Glyceraldehyde-3-phosphate (G3P)------> Pyruvate
A. cytoplasm
B. nucleus
C. mitochondria
D. none of the above
A

A. The oxidation of G3P into pyruvate occurs during the glycolysis stage of cellular respiration. Glycolysis occurs in the cytoplasm

32
Q
Which would yield an endothermic reaction?
A. TG=298, T=298, TS= -1
B. TG= -298, T=298, TS= -2
C. TG= -298, T=0, TS=1
D. none of them
A

D. The free energy change of a reaction, TG, is equal to the difference between TH, the change in enthalpy, and the product of the temperate, T, with the change in entropy, TS, of the system: TG=TH-TTS. Solve for TH in each case: A=0, B= -894, C= -298

33
Q

_____ law sates that the _____ is the sum of ______ in a gas compound.
A. Dalton’s, partial pressure, total pressure
B. Henry’s, partial pressure, total pressure
C. Dalton’s, total pressure, partial pressures
D. Henry’s, total pressure, partial pressures

A

C. Dalton’s law states that the total pressure of a gaseous compound is the sum of the partial pressures of each gas making up the compound

34
Q
What effect would doubling the volume and temperature of an ideal gas have on its pressure?
A. double the pressure
B. half the pressure
C. make the pressure zero
D. no effect
A

D. The ideal gas law states: pV=NRT, where p is pressure, V is volume, N is the amount, R is the ideal gas constant, and T is the gas’s temperature. Doubling the volume V=2V, and doubling the temperature, T=2T, will have not alter the pressure because the 2’s on both sides of the equation will cancel, yielding the original pressure

35
Q
What is the molecular formula of acetic acid?
A. C2H4O2
B. C3H6O
C. CH2O
D. CHO
A

A. Acetic acid is often produced by way of methanol carbonylation wherein methanol, CH3OH, reacts with carbon monoxide, CO, to produce acetic acid, CH3COOH. Rewriting in terms of the molecular formula gives you C2H4O2

36
Q
The hybridization of the oxygen in CO2 is:
A. s
B. sp
C. sp2
D. sp3
A

C. An analysis of the Lewis structure for CO2 shows a steric number of 2 for the carbon atom because of the 2 oxygen atoms attached (no lone pairs). Each oxygen atom has 2 lone pairs and is connected with the carbon atom, so a steric number of 3, and consequently, a hybridization of sp2

37
Q
An enzyme reaction reaches \_\_\_\_\_ at \_\_\_\_\_.
A. Vmax, Km
B. Vmax, 1/2Km
C. 1/2Vmax, Km
D. 1/2Vmax, 1/2Km
A

C. Vmax is the maximum rate at which an enzymatic reaction can occur. Km is the substrate concentration yielding a reaction rate that is half of the maximum reaction rate.

38
Q
Which of the following would show a peak at 2190 cm-1?
A. alkane
B. alkene
C. alkyne
D. ketone
A

C. Alkynes, which possess a carbon to carbon triple bond, correspond with frequencies that range from 2300 cm-1 to 2100 cm-1. Alkanes, alkenes, and ketones involve C-H, C–C, and C–O bonds, respectively. None of the other bonds correspond to frequencies near 2190 cm-1

39
Q
The \_\_\_\_\_\_ is the \_\_\_\_\_\_ at which a protein has no net charge.
A. pH, pKa
B. pl, pKa
C. pH, pl
D. pl, pH
A

D. A protein will have no net charge when its composite amino acids taken together yield no overall charge. The pl, or isoelectric point, is the pH at which a molecule, in this case protein, carries no net charge

40
Q
FADH2 is classified as which of the following?
A. oxidizing agent
B. reducing agent
C. intermediate
D. none of the above
A

B. In cellular respiration, FADH2 acts as an electron carrier and donor. Reducing agents are those that lose electrons during a reaction. Oxidizing agents are those that gain electrons during a reaction. Oxidation of FADH2 results in FAD+

41
Q
Which of the following has the largest bond order?
A. O2
B. NO3-
C. NO2+
D.CN-
A

D. Bond order for diatomic molecules is found by determining the type of bonds between the 2 atoms. In cases where there are more than two atoms involved, count the number of bonds, then count the number of bond groups between atoms, then calculate the ratio of the number of bonds to the total number of bond groups. The Lewis structure for A shows a double bond between oxygen atoms, and its bond order is 2. B shows a double bond between N and O, and 2 single bonds between N and O

42
Q
What is the osmotic pressure of a 2M NaCl solution at 0 degrees C?
A. 44.8 atm
B. 45.5 atm
C. 0 atm
D. 97 atm
A

A. Calculate osmotic pressure using pi=MRT, where pi is pressure, M is the molar concentration of the dissolved solution, R is the ideal gas constant, and T is the temperature in Kelvins.

43
Q
Which compound forms when acetyl-CoA enters the TCA cycle?
A. oxaloacetate
B. acetic acid
C. citrate
D. FADH2
A

C. Prior to the TCA cycle, glycolysis functions to breakdown glucose into pyruvate which is then decarboxylated and turned into acetyl-CoA. Acetyl-CoA combines with oxaloacetate to make citrate, which marks the start of the TCA cycle

44
Q
Which of the compounds has the lowest boiling point?
A. CH3(CH2)2CH3
B. CH3CH(CH3)2
C. CH3(CH2)2CH2OH
D. CH3CH(CH3)OH
A

B. When comparing boiling points among compounds, consider these 3 generalities: (1) boiling point increases relative to the strength of the intermolecular forces present in the compound; ionic bonding is stronger than hydrogen bonding is stronger than dipole dipole bonding is strong than Van der Waals forces. (2) Boiling point also increases as the molecular weight of the compound increases. (3) Branching of the compound decreases the boiling point (mitigation of Van der Waals forces).

45
Q
Which law states that the volume of a gas is proportional to the number of moles of a gas at constant temperature and pressure?
A. Dalton's Law
B. Avogadro's Law
C. Charles's Law
D. Henry's Law
A

B. Avogadro’s Law relates the volume of a gas to the amount of substance of gas present: V=nk, where V is the volume of the gas, n is the number of moles of the gas, and k is the constant equal to RT/P where R is the universal gas constant, T is temperature in Kelvins, and P is the pressure

46
Q
How many sigma bonds does HCCH have?
A. 1
B. 2
C. 3
D. 4
A

C. Recall that single bonds are always sigma bonds, double bonds consist of a sigma bond and a pi bond, and triple bonds contain one sigma bond and two pi bonds. HCCH contains 2 C-H bonds and 1 C-C triple bond. So, 2 C-H bonds gives 2 sigma bonds, and another sigma bond from the triple bond equals 3 sigma bonds

47
Q
Which of the following reactions creates an alkene?
A. addition
B. substitution
C. hydration
D. dehydration
A

D. Dehydration involves the loss of an H2O molecule from the reacting molecule. Recall that the general structure of alcohols is: CnH2n+1OH. The removal of H2O from an alkyl group results in a molecule of the general form

48
Q
The viscosity of a liquid:
A. increases with decreasing temperature
B. increases with increasing temperature
C. decreases with decreasing temperature
D. is independent of temperature
A

A. A liquid’s viscosity, or its resistance to flow, changes with a change in temperature. As a liquid’s temperature increases, bonds within it break and the molecules in the liquid cna move more freely and easily, decreasing its viscosity. Likewise, if the temperature decreases, molecules have more of an opportunity to form bonds which then decreases the liquid’s fluidity, increasing its viscosity