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Day 1 > PCP-Diagnostic Exam > Flashcards

PCP-Diagnostic Exam Flashcards

1
Q

The total number of electrons at the fourth energy level is
A. 2
B. 8
C. 18
D. 32

A

D. 32

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2
Q

The halogen with the highest electronegativity is
A. fluorine
B. chlorine
C. bromine
D. iodine

A

A. fluorine

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3
Q

The geometry of the SO3 molecule is best described as
A. linear
B. trigonal planar
C. tetrahedral
D. bent

A

B. trigonal planar

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4
Q

Only two isotopes of copper are present in naturally occurring copper: 62Cu (62.9298 u) and 65Cu (64.9278 u). Calculate the percent composition of naturally occurring 62Cu using atomic mass of 63.546 u.
A. 69.17%
B. 30.83%
C. 46.65%
D. 53.35%

A

A. 69.17%

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4
Q

If 5.0 E 10 barium (Ba) atoms could be arranged side by side, they would form a straight line measuring 22 m. What is the diameter of Ba in pm? In A?
A. 44 pm, 0.44 A
B. 4.4. pm, 440 A
C. 440 pm, 4.4. A
D. 220 pm, 2.2. A

A

C. 440 pm, 4.4. A

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5
Q

Maleic acid contains 41.4% carbon, 3.47% , and 55.1% oxygen by weight. A 0.050-mole sample of this sample of this compound weighs 5.80 g. What is the molecular formula of maleic acid?
A. CHO
B. C2H2O2
C. C3H3O
D. C4H4O4

A

D. C4H4O4

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6
Q

A special-purpose piece of laboratory glassware, called pycnometer, is used to measure liquid densities. It has a volume of 25 cc, and a mass of 17.24 g when it is full of air. When filled with a liquid of unknown density, its mass = 45.0 g. What is the density of this liquid?
A. 1.11 g/mL
B. 1.25 g/mL
C. 1.42 g/mL
D. 1.55 g/mL

A

A. 1.11 g/mL

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7
Q

An 8.24-gram sample of a hydrated salt is heated until it has a constant mass of 6.20 grams. What was the percent by mass of water contained in the original container?
A. 14.1%
B. 32.9%
C. 24.8%
D. 75.2%

A

C. 24.8%

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8
Q

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25°C. Calculate the molarity of a solution of acetic acid made by dissolving 10.0 mL of glacial acetic acid at 25°C in enough water to make 100 mL of solution.
A. 1.665 M
B. 1.747 M
C. 100.0 M
D. 104.9 M

A

B. 1.747 M

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9
Q

Calculate the molarity of a 5.00 ppm Ca(NO3)2 solution. Ca=40; N=14; 0=16
A. 2.56 E-6 M
B. 2.56 E-5 M
C. 3.05 E-5 M
D. 3.05 E-6 M

A

C. 3.05 E-5 M

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10
Q

How many milliliters of water must be added to 5 mL of 12 M HCl solution to make a 3 M HCl solution?
A. 10 mL
B. 15 mL
C. 20 mL
D. 25 mL

A

B. 15 mL

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11
Q

What type of colloid is mayonnaise?
A. Aerosol
B. emulsion
C. solid foam
D. sol

A

B. emulsion

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12
Q

A current of 0.1000 ampere is passed through a copper sulphate solution for 10 minutes using platinum electrodes. Calculate the number of grams of copper deposited at the cathode from CuSO4 solution.
A. 0.01975 g
B. 0.0243 g
C. 0.0385 g
D. 0.0457 g

A

A. 0.01975 g

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13
Q

The wavelength of a beam is 24 micrometer. What is its wave number?
A. 380/cm
B. 417/cm
C. 440/cm
D. 490/cm

A

B. 417/cm

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14
Q

A fossil fern containing 0.110 lbm of carbon is carbon dated to determine its age. The decay rate of C-14 in the fossil is 191 decays/min. How old is the fern? (The half-life of C-14 is 5730 years, and the rate decay of C-14 in a living organism is 6800 decays/min-lbm C.)
A. 7290 yrs
B. 11300 yrs
C. 14100 yrs
D. 23800 yrs

A

B. 11300 yrs

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15
Q

Consider the reaction Pb2+(aq) + 2Cl- (aq) → PbCl2 (s) H= -22.53 kJ/mol. Calculate H when 0.230 mol of PbCl2 (s) is dissolved in water.
A. 5.18 kJ
B. -5.18 kJ
C. 22.5 kJ
D. -22.5 kJ

A

A. 5.18 kJ

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16
Q

At what temperature do the Celsius scale and Fahrenheit scale readings have the same numerical value?
A. 40°C or 40°F
B. 32°C or 32°F
C. -40°C or -40°F
D. -100°C or 100°F

A

C. -40 C or -40 F

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17
Q

Two gas storage bulbs are at the same temperature. The 1 L bulb contains 0.50 atm of helium and the 2 L bulb contains 1 atm nitrogen. The valves connecting the two bulbs are opened and they are connected through a negligible volume. The pressure in the bulbs after they have pressure equilibrated and are at the initial temperature is
A. 1.50 atm
B. 0.67 atm
C. 0.50 atm
D. 0.84 atm

A

D. 0.84 atm

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18
Q

A volume of dry gas measures 85 mL at 21°C and 758 mmHg. What volume would this gas occupy if collected over water at 755.5 mmHg at 25°C?
A. 85 mL
B. 86.5 mL
C. 69 mL
D. 83.2 mL

A

C. 69 mL

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19
Q

A mixture consisting of 0.100 mol N2, 0.05 mol O2, 0.20 mol CH4, and an unknown amount of CO2 occupied a volume of 9.6 L at 27°C and 1 atm pressure. How many moles of CO2 are there in this sample?
A. 0.04 mol
B. 0.05 mol
C. 0.10 mol
D. 0.39 mol

A

A. 0.04 mol

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20
Q

Helium and argon are monoatomic gases and their atomic weights are 4 and 40 respectively. Under identical conditions helium will diffuse through a semipermeable membrane
A. 3.16 times as fast as argon
B. 1.58 times as fast as argon
C. 7.32 times as fast as argon
D. 10 times as fast as argon

A

A. 3.16 times as fast as argon

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21
Q

At 20°C and one atmosphere, one liter of water will absorb 0.043 g of oxygen or 0.19 g of nitrogen. Atmospheric air is 20.9% oxygen by volume, and the remainder is assumed to be nitrogen. What mass of oxygen will be absorbed by one liter of water exposed to 20°C air at one atmosphere?
A. 0.009 g
B. 0.150 g
C. 0.23 g
D. 0.043 g

A

A. 0.009 g

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22
Q

At 0°C the average velocity of methane molecules in air is 600 m/s. what is the total kinetic energy of 1.00 mol of methane molecules moving at this speed?
A. 4.78 E-21 J
B. 2.88 E 3 J
C. 5.76 E 3 J
D. 1.80 E 5 J

A

C. 5.76 E 3 J

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23
Q

The molecular diameter of CO is 3.19×10-6 cm, at 300K and pressure of 100 mmHg. What is the mean free path of the gas in cm?
A. 6.06×10-6
B. 6.86×105
C. 6.86×10-3
D. 2.86×10-4

A

C. 6.86×10-3

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24
Q

What is the pH of a 0.30 M s olutionof benzoic acid, Ka = 6.6E -5?
A. 0.52
B. 2.4
C. 4.7
D. 4.2

A

C. 4.7

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25
Q

Calculate the pH of an aqueous buffer solution which contains 0.100 mol/L NH3 and 0.200 mol/L NH4Cl.
A. 9
B. 8.5
C. 7.0
D. 10

A

A. 9

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26
Q

At equilibrium, a 1-liter reactor contains 0.3 mol of A, 0.1 mol of B and 0.6 mol 0f C, according to the equation: A + B → C. If 0.4 mol of A was added, how many moles of A was left under equilibrium was re-established?
A. 0.65
B. 0.05
C. 0.35
D. 0.70

A

A. 0.65

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27
Q

The solubility of barium carbonate is 1.4 E-3 g/ 100 mL solution. Determine its Ksp.
A. 5 E-9
B. 4 E-7
C. 4.5 E-8
D. 5.6 E-1

A

A. 5 E-9

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28
Q

Who discovered positron?
A. Anderson
B. Pauli
C. Heisenberg
D. Bohr

A

A. Anderson

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29
Q

An atomic face-centered cubic central crystal is 3.92 angstrom on an edge and has a density of 21.5 g/cm3. What is its atomic weight?
A. 195
B. 207
C. 48.8
D. 108

A

A. 195

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30
Q

Magnesium is obtained from
A. Sea shells
B. bentonite
C. sea water
D. corals

A

C. sea water

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31
Q

How many mililiters of 0.01000 N Ba(OH)2 are theoretically required to titrate 0.03000 g of H3AsO4 to the formation of Ba(H2AsO4)2?
A. 16.4 mL
B. 17.6 mL
C. 18.9 mL
D. 21.14 mL

A

D. 21.14 mL

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32
Q

Ethers are formed from condensation reactions between
A. alcohols and aldehydes
B. others and acids
C. aldehydes and acids
D. alcohols and acids

A

D. alcohols and acids

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33
Q

What is the name of the following compound?
CH3
|
CH–CH2–CH3
|
|
CH3–CH2–CH–CH3

A. 3,4-dimethylhexene
B. 3-butylbutane
C. 3-methyl 4-ethylpentane
D. 3,5-octane

A

A. 3,4-dimethylhexene

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34
Q

Which of the following aromatic hydrocarbons is consist of two benzene rings?
A. toluene
B. naphthalene
C. anthracene
D. phenanthrene

A

B. naphthalene

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35
Q

Which of the following tests will distinguish 1-propanol from 2-propanol?
A. Fehling’s test
B. Tollen’s test
C. Benedict’s test
D. Lucas test

A

D. Lucas test

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36
Q

A carboxylic acid which contributes to the strong odor of rancid butter and other fats.
A. caproic acid
B. acetic acid
C. lactic acid
D. butyric acid

A

D. butyric acid

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37
Q

Which of the following is an acid found in milk?
A. lactic acid
B. tartaric acid
C. malic acid
D. citric acid

A

A. lactic acid

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38
Q

Ascorbic acid is
A. vitamin C
B. vitamin D
C. tocopherol
D. vitamin E

A

A. vitamin C

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39
Q

Retinal, retinol, and retinoic acid are stable form of
A. vitamin A
B. vitamin C
C. vitamin B
D. vitamin D

A

A. vitamin A

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40
Q

Which of the following is a ketose?
A. fructose
B. glucose
C. sucrose
D. maltose

A

A. fructose

41
Q

The vitamin responsible for blood clotting is
A. A
B. B
C. K
D. E

A

C. K

42
Q

For an enzyme that displays Michaelis-Menten kinetics, the reaction velocity (as a fraction of Vmax) observed at [S]= 2 KM will be
A. 0.09
B. 0.33
C. 0.66
D. 0.91

A

C. 0.66

43
Q

In the Lineweaver-Burk double reciprocal plot the slope is equal to
A. 1/[S]
B. 1/V
C. Km/Vmax
D. 1/Vmax

A

C. Km/Vmax

44
Q

Which of the following amino acid is basic?
A. lysine
B. aspartic acid
C. tyrosine
D. alanine

A

A. lysine

45
Q

Which of the following amino acid is polar?
A. glutamine
B. arginine
C. Proline
D. Valine

A

A. glutamine

46
Q

Which of the following amino acid is nonpolar?
A. glutamic acid
B. leucine
C. cysteine
D. serine

A

B. leucine

47
Q

Calculate the “exact” alkalinity (in milligrams per liter as CaCO3) of a water containing 120 mg/L of bicarbonate ion and 15 mg/L of carbonate ion, at a pH of 9.43.
A. 110.5 mg/L
B. 116.2 mg/L
C. 123.4 mg/L
D. 128.9 mg/L

A

C. 123.4 mg/L

48
Q

A surface water primarily used for contact recreation such as bathing, etc.
A. Class A
B. Class SA
C. Class B
D. Class AA

A

C. Class B

49
Q

Also known as The Clean Air Act of the Philippines of 1999.
A. RA 8749
B. PD 984
C. RA 6969
D. PD 600

A

A. RA 8749

50
Q

The ionic strength of 0.1 M solution of ferrous sulphate is
A. 0.75
B. 0.50
C. 1.50
D. 0.40

A

D. 0.40

51
Q

A sanitary landfill is 210,000 square meters in area and 2 m deep. The daily loading of garbage is 800 m3/day. What is the life at the landfill in years if the garbage is compacted in the landfill with twice its loading density.
A. 3 years
B. 13.3 years
C. 2.88 years
D. 16.3 years

A

C. 2.88 years

52
Q

Glutamic acid (C5H9O4N) is used as one of the reagents for standard to check the BOD test. Determine the theoretical oxygen demand of 150 mg/L of glutamic acid. Assume the following reactions apply:
C5H9O4N + 4.5 O2 → 5CO2 + 3H2O + NH3
NH3 + 2O2 → NO3- + H+ + H2O
A. 180 mg/L
B. 190 mg/L
C. 198 mg/L
D. 212 mg/L

A

D. 212 mg/L

53
Q

If the five-day BOD of a waste is 220 mg/L and the ultimate BOD is 320 mg/L, what is the rate constant?
A. 0.142/day
B. 0.178/day
C. 0.210/day
D. 0.233/day

A

D. 0.233/day

54
Q

A solution of an unknown non volatile nonelectrolyte was prepared by dissolving 0.250 g of the substance in 40 g of carbon tetrachloride. The boiling point of the resultant solution was 0.357°C higher than that of the pure solvent. Calculate the molar mass of the solute. Molal boiling point elevation constant for carbon tetrachloride is 5.02°C/ molal.
A. 64
B. 74
C. 68
D. 88

A

D. 88

55
Q

184 grams of ethanol is mixed with 1 gmol glycerol. What is the vapour pressure of the resulting solution if the vapor pressure of ethanol at the working temperature is 200 mmHg? Assume glycerol is non-volatile.
A. 176 mmHg
B. 182 mmHg
C. 160 mmHg
D. none of these

A

C. 160 mmHg

56
Q

If ethanol and methanol are mixed 50/50 by weight at 60°C, and the solution assumed ideal, the composition of the vapor above the solution is
A. 28% ethanol, 72% methanol
B. 72% ethanol, 28% ethanol
C. 59% ethanol, 41% methanol
D. 41% ethanol, 59% methanol

A

A. 28% ethanol, 72% methanol

57
Q

A solution with only 12 g of unknown polymer per liter of solution at 25°C has an osmotic pressure of 12.1 torr. What is the molar mass of the polymer?
A. 18,400 g/mol
B. 24.2 g/mol
C. 9,200 g/mol
D. 1533 g/mol

A

A. 18,400 g/mol

58
Q

Use the van der Waals equation of state to calculate the pressure exerted by exactly 1 mol of gaseous ammonia, NH3, held at a temperature of 1000 K in a vessel of volume 2.50 dm3. The values of the van der Waals parameters for ammonia are a= 4.225 atm dm6 mol-2 and b= 3.71 ×10-2 dm3 mol-1.
A. 3.33 kPa
B. 3.31 MPa
C. 1970 Pa
D. 224 kPa

A

B. 3.31 MPa

59
Q

18.7 g of unknown acid is reacted with the zinc to produce 800 cc of the gas at STP. What is the equivalent weight of the acid?
A. 624 B. 173 C. 262 D. 131

A

C. 262

60
Q

Suppose you are given a gaseous compound for which the formula is C_XH_2X-2 at the same temperature and pressure at which oxygen weighs 4.8 grams per liter, the unknown gas weighs 8.10 g/L. What is the formula of the compound?
A. C2H2
B. C3H6
C. C4H6
D. C4H10

A

C. C4H6

61
Q

When evacuated or empty a gas density bulb weighs 29.3215 grams. First, CO2 gas was used to fill the bulb at 40 deg C and 1.0 atm P and it weighed 30.0079. The bulb was then evacuated and filled with a mixture of CO and CO2 under the same temperature and pressure. With this mixture the bulb weighed 29.9332. Determine the % of CO in the mixture.
A. 21
B. 29
C. 32
D. 15

A

B. 29

62
Q

PCl5 (g) dissociates into PCL3 (g) and Cl2 (g) when heated at 250°C and 1 atm. If the density of the gas mixture at equilibrium is 4.4 g/L, the fraction of PCl5 dissociated is
A. 0.103
B. 0.328
C. 0.725
D. 0.209

A

A. 0.103

63
Q

The alcohol in “gasohol” burns according to the following equation: C2H5OH + 3O2 → 2CO2 + 3H2O. How many grams of CO2 are produced when 3 g of C2H5OH are burned in this way?
A. 6.00 g
B. 44.0 g
C. 0.130 g
D. 5.74 g

A

D. 5.74 g

64
Q

Silicon carbide, SiC, is commonly known as carborundum. This hard substance, which is used commercially as an abrasive, is made by heating SiO2 and C to high temperatures: SiO2(s) + 3C(s) → SiC(s) + 2CO(g). How many grams of SiC can form when 3.00 g of SiO2 and 4.50 of C are allowed to react?
A. 2.00 g
B. 3.00 g
C. 5.01 g
D. 15.0 g

A

A. 2.00 g

65
Q

Propane is a hydrocarbon with the formula C3H8 that is used as a bottled gas. How many liters of oxygen are needed to burn 1 L of propane gas? Assume all volumes to be measured at the same temperature and pressure.
A. 5 L
B. 6 L
C. 3 L
D. 2 L

A

A. 5 L

66
Q

Propane is a hydrocarbon with the formula C3H8 that is used as a bottled gas. How many liters of carbon dioxide are produced by the reaction? Assume all volumes to be measured at the same temperature and pressure.
A. 5 L
B. 6 L
C. 3 L
D. 2 L

A

C. 3 L

67
Q

Dulong and Petit, French physicist, observed in 1819 that the product of specific heat, J/g-C, and atomic weight, g/mol/, is approximately equal to 26 J/mol-C for many solid elements. A 135-g sample of a metal is heated to 80°C the immersed into a calorimeter containing 75 g of water at 22°C. The system equilibrates and the temperature of the water rises to 25.1°C. What is the specific heat of the metal?
A. 0.0075 J/g-C
B. 0.042 J/g-C
C. 0.13 J/g-C
D. 1.005 J/g-C

A

C. 0.13 J/g-C

68
Q

Dulong and Petit, French physicist, observed in 1819 that the product of specific heat, J/g-C, and atomic weight, g/mol/, is approximately equal to 26 J/mol-C for many solid elements. A 135-g sample of a metal is heated to 80°C the immersed into a calorimeter containing 75 g of water at 22°C. The system equilibrates and the temperature of the water rises to 25.1°C. What is the specific heat of the metal?
From the data in the problem #68, is the metal copper, gold, tin, or iron?
A. copper
B. gold
C. tin
D. iron

A

B. gold

69
Q

A 1-kg iron bar [c=0.11 kcal/kg-°C] at 100°C is placed in 3.0 kg water at 15°C. The temperature of the water increases by
A. 0.7°C
B. 3°C
C. 5°C
D. 18°C

A

B. 3°C

70
Q

With the pressure approaching zero, compressibility factor approaches
A. Zero
B. unity
C. infinity
D. constant

A

B. unity

71
Q

If an initial volume of an ideal gas is compressed to one-half its original volume and to twice its original temperature, the pressure ______.
A. Doubles
B. halves
C. quadruples
D. triples

A

C. quadruples

72
Q

Consider the reaction: 4NH3 + 7O2 → 4NO2 + 6H2O. At a certain instant the initial rate of disappearance of the oxygen gas is X. What is the value of the appearance of water at the same instant?
A. 1.2X
B. 1.1X
C. 0.86X
D. 0.58X

A

C. 0.86X

73
Q

For ammonia synthesis reaction, N2 + 3H2 → 2NH3, if the rate of reaction with respect to N2 is X, what is the rate with respect to H2 in terms of x?
A. x/3
B. 2x
C. 3x
D. 2x/3

A

C. 3x

74
Q

What is the reaction rate constant, K, for the third order reaction?
A. (L/mol)/s
B. (L/mol)/s2
C. (L/mol)2/s
D. (L/mol)3/s

A

C. (L/mol)2/s

75
Q

What law governs the rate of reaction of a substance?
A. Law of conservation of mass
B. Arrhenius Law
C. law of mass action
D. Avogadro’s Law

A

C. law of mass action

76
Q

If Ca is plotted versus time and a straight line is observed, the reaction is said to be
A. First order
B. second order
C. zero order
D. fractional order

A

C. zero order

77
Q

The overall order of reaction for the elementary reaction A + 2B → C is
A. 0
B. 1
C. 2
D. 3

A

D. 3

78
Q

The reaction is known to be first order in A. A straight line will be obtained by plotting
A. log CA versus time
B. log CA versus reciprocal time
C. CA versus time
D. 1/CA versus time

A

A. log CA versus time

79
Q

If the reaction 2A → B + C is second order, which of the following plots will give a straight line?
A. CA
2 vs time
B. 1/CA vs time
C. log CA vs time
D. CA vs time

A

B. 1/CA vs time

80
Q

Which statement about orbitals is false?
A. Orbitals are regions of space where electrons are found.
B. Orbitals may contain up to two electrons.
C. Orbitals are filled in order of decreasing energy.
D. Orbitals of equivalent energy are half filled before adding two electrons to any one of them

A

C. Orbitals are filled in order of decreasing energy.

81
Q

Which fractions of petroleum distils are at the highest temperature?
A. Gasoline
B. gases
C. fuel oil
D. kerosene

A

C. fuel oil

82
Q

How many atoms are there in a molecule of naphthalene?
A. 10
B. 20
C. 18
D. 24

A

C. 18

83
Q

Plastic used for synthetic leather.
A. PVC
B. PE
C. PS
D. PTFE

A

A. PVC

84
Q

The least number of atoms in alkynes is
A. 4
B. 6
C. 5
D. 7

A

A. 4

85
Q

Ethylene glycol is
A. Triol
B. ester
C. diol
D. pheno

A

C. diol

86
Q

Oxidation of a primary alcohol yields
A. Ketones
B. ethers
C. aldehydes
D. esters

A

C. aldehydes

87
Q

Which of the following represents an acceptable set of quantum number?
A. 2,2,-1,-1/2
B. 1,0,0,1/2
C. 5,-4,-3,1/2
D. 3,3,3,-1/2

A

B. 1,0,0,1/2

88
Q

Which one of the following is an impossible set of quantum number for an electron in an atom?
A. 2,2,-1,-1/2
B. 1,0,0,1/2
C. 5,-4,-3,1/2
D. 3,3,3,-1/2

A

D. 3,3,3,-1/2

89
Q

Deuterium is an isotope of _______.
A. Hydrogen
B. oxygen
C. nitrogen
D. helium

A

A. Hydrogen

90
Q

The nuclei of tritium atom would contain ____ neutrons.
A. 1
B. 2
C. 3
D. 4

A

B. 2

91
Q

If the following reaction were at equilibrium in a closed vessel at a controlled temperature, what would be the effect of adding more CO2 to the reaction vessel and permitting the reaction to approach equilibrium again?
CO + H2O ⟷ CO2 + H2
A. The concentrations of CO, H2O, and H2 would all increase.
B. The concentrations of CO, H2O, and H2 would all decrease.
C. The concentrations of CO and H2O would decrease and the concentration of H2 would increase.
D. The concentrations of CO and H2O would increase and the concentration of H2 would decrease

A

D. The concentrations of CO and H2O would increase and the concentration of H2 would decrease

92
Q

The following reactions are known to occur in the body: CO2 + H2O ⟷ H2CO3 H + + HCO3-, if CO2 escapes from the system.
A. pH will decrease
B. hydrogen ion concentration will diminish
C. H2CO3 concentration will be unaltered
D. the forward reaction will be promoted

A

B. hydrogen ion concentration will diminish

93
Q

What type of covalent bonds link the amino acids in protein?
A. hydrogen bonds
B. ionic bonds
C. peptide bonds
D. glycosidic bonds

A

C. peptide bonds

94
Q

Which amino acid is very important for optimal immune function and exhibits a reduced plasma concentration during heavy training?
A. Glycine
B. glutamine
C. isoleucine
D. leucine

A

B. glutamine

95
Q

In a Michaelis-Menten enzyme mechanism, what substrate concentrations (relative to Km) are needed for the reaction rate to be 0.9 times Vmax?
A. (1/9)Km
B. (1/3)Km
C. 1.0Km
D. 9.0Km

A

D. 9.0Km

96
Q

Atoms of which element have the highest first ionization energy?
A. Calcium
B. potassium
C. sodium
D. magnesium

A

D. magnesium

97
Q

Transition elements are found in the
A. d & f energy level
B. s energy level
C. d energy level
D. p energy leve

A

A. d & f energy level

98
Q

Which of the following is a metalloid?
A. Ge
B. Al
C. Be
D. Zn

A

A. Ge

99
Q

The mass defect in a particular nucleus is
A. the difference between the mass of the protons and the mass of the neutrons
B. the mass that has been converted into nuclear binding energy
C. the difference between the calculated and the exponential nuclear mass which is the mass that has been converted into nuclear binding energy
D. the experimental error in determining the nuclear mass

A

C. the difference between the calculated and the exponential nuclear mass which is the mass that has been converted into nuclear binding energy

Day 1 (10 decks)

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