MDCAT CHEMISTRY-Fundamental Concepts (SMART INSTITUTE)

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MDCAT Chemistry Challenge

Test your knowledge of fundamental chemistry concepts with our MDCAT Chemistry quiz! This quiz is designed to challenge students and enthusiasts alike, covering a range of topics from stoichiometry to mass spectrometry.

Get ready to dive into immersive questions that will help you solidify your understanding of chemistry. Whether you're preparing for exams or simply looking to refresh your knowledge, this quiz is for you!

  • Multiple choice format
  • Comprehensive coverage of key concepts
  • Ideal for MDCAT preparation
60 Questions15 MinutesCreated by ExploringAtom427
01-The stoichiometric calculations for a chemical reaction results in
Actual yield
Percentage yield
Theoretical yield
Selectivity
02-Mass spectrometry is used to determine the
Number of isotopes of an element
Relative abundance of isotopes
Relative isotopic mass
All of these
03. 1 gram molecule refers to amount in grams
Equivalent to 1 mole of an atom
Equivalent to 1 mole of a molecule
Equivalent to 1 mole of an ionic species
Of an ionic compound
04-Number of H+ ions when 0.1 mole of sulfuric acid is completely ionized in water:
4 x NA
1 x NA
2 x NA
2 x 6.022 x 10^22
05. 1 gram formula refers to:
Amount in grams equivalent to 1 mole of an atom
Amount in grams equivalent 1 mole of a covalent compound
Amount in grams equivalent to 1 mole of an ionic compound
Amount in grams equivalent to 1 mole of an ion
06-How many electrons have to be removed to ionize 1.0 x 10^6 moles of Ne atoms to Ne+ ions in a neon advertising tube.
6.02 x 10^23 / 1.0 x 10^-6
1.0 x 10^-6 x 6.02 x 10^23 / 20.2
1.0 x 10^-6 x 6.02 x 10^23
1.0 x 10^-6 x 6.02 x 10^23 / 9.65x110^-1
07-One mole of SO2 contains
6.022 x 10^23 atoms of oxygen
6.022 x 10^23 atoms of sulfur
18.1 x 10^23 molecules of SO2
4g molecule of SO2
08-Mg reacts with HCl as per the following reaction 
Mg(s) + 2HCl(aq)  →  MgCl2(aq) + H2 (g)
Given that;Mg=21g and HCl=21g, the excess reactant is;
Mg
HCl
Both are in stoichiometric amounts
None of these
09. 5604 cm3 of H2 gas at STP contains atoms of hydrogen
6.02 x 10^23
3.01 x 10^23
2.6 x 10^22
1.50 x 10^23
10-Number of moles present in 0.6 gram of silica is
0.01 mole
0.064 mole
0.044 mole
0.054 mole
11-Gram atoms of hydrogen in 5.5g H2
5.50
2.25
5.45
2.20
12- % of Nitrogen in urea (NH2CONH2)
82.35
35
46.6
55.56
13-One mole of potassium chlorate is thermally decomposed and excess of aluminum is burnt in gaseous mixture. How many moles of aluminum oxide are formed?
Respective equations are given as 
2KClO3 (MnO2)→ 2KCl + 3O2     
4Al +3O2 → 2Al2O3
1.0
2.0
1.5
3.0
14-In a mass spectrometer, increasing the electric field with constant magnetic field results in
Increased radius "r"
Increased ionization energy
Decreased radius "r'
None of above
15-When 0.5 moles of Al2(SO4)3 are dissolved in water, total number of particles produced
1.2 x 10^23
3.0 x 10^23
1.5 x 10^24
2.5 x 10^23
16. 4 g of an unknown mass gas occupies 5.6 dm3 volume, at S.T.P the gas is:
SO2
O2
CH4
H2S
17. The mass of one mole of Mg atoms is 24g. What is the mass of one Mg atom in grams?
NA
3.99 x 10^^-23
6.02 x 10^-23
3.99 x 10^23
18-WOF contains 1 mole of the stated particles:
Chlorine molecules in 35.5 g of Chlorine gas
Electrons in 1 g of hydrogen gas
Hydrogen ions in 1 dm3 of 1 mol dm-3 aqueous sulfuric acid
Oxygen atoms in 22.4 dm3 of oxygen gas at STP
19-During combustion analysis, which one is used for absorbing carbon dioxide
50% KOH solution
Mg(ClO4)2
5% KOH
Silica gel
20. 1 amu=?
1.661 x 10^-27 g
1.661 x 10^-24 kg
1.661 x 106-19 kg
1.66 x 10^-21 mg
21-Molecular ions are produced in mass spectrometer. Which type of molecular ions formed more abundantly
Negatively charged
Positively charged
H+ ions
Equal positive and negative ions
22-The height of the peak in the mass spectrum shows
Number of isotopes
Mass number
Relative abundance
Number of protons
23-The separation of different isotopes in the mass spectrometer is done on the basis of:
Different amounts of positive charge on each ion
Different m/e
Different e/m value
Velocities of the ions
24-A compound contains 50% sulfur and 50% oxygen by mass. The empirical formula of the compound is:
S2O3
SO3
SO2
SO
25-Equal volumes of CO and N2 are taken in identical conditions. The correct relationship between masses of two gases is;
CO
N2
CO=N2
All of These
26-The approximate number of molecules present in 3 g of H2O is
3 x 10^23
3 x 6.01 x 10^23
1 x 10^23
2 x 10^23
27-The mass of one molecule of O2 is
6.02 x 10^23 / 32
32 g
0.32 g
32 / 6.02 x 10^23
28-Combustion analysis is performed for the determination of
Molar mass of the compound
Structural formula of the substance
Empirical formula of the compound
Mass of the halogens present in organic compounds
29.The largest number of molecules are present in
3.6 of H2O
2.8 g of CO
4.6 g of C2H5OH
5.4 g of N2O5
30-The number of moles of CO2 which contain 16g of Oxygen
0.25
1.00
0.50
1.50
31-Haemoglobin molecule is how many times heavier than He atom.
68,000 times
17,000 times
34,000 times
1700 times
32-Atoms having same mass number but different atomic numbers are called
Isotopes
Isobars
Isotones
Isomers
33- 40 g of Calcium is
1 gram of Ca
1 gram atom of Ca
1 atom of Ca
1 gram ion of Ca
34-Amount of Oxygen in grams which contains 1.5 x 10^22 molecules
0.08
0.80
80
1280
35-What volume of Oxygen is required for complete combustion of 5 cm3 C2H2
2 cm3
12.5 cm3
5 cm3
13.5 cm3
36-How many atoms of carbon are present in 3.42 g
6.02 x 10^22
7.2 x 10^22
3.6 x 10^23
1.8 x 10^23
37-Absorption of CO2 in KOH solution during combustion analysis is:
Chemical change
Neither chemical nor physical change
Physical change
CO2 absorbed in Mg(ClO4)2
38- 10 moles of HCl is added to excess to Magnesium and forms 4 moles of Hydrogen gas. Percentage yield is
40
60
80
100
39-If you have 3.5 moles of Hydrogen and 5 moles of Nitrogen to produce Ammonia. How much Ammonia is produced?
34.08 g
39.6 g
17.04
None of these
40-Empirical formula of Vitamin C is:
C3H4O3
C4H8O7
C3H6O3
C6H12O6
41-Number of electrons in half mole of Na+
10
5.5 NA
5
5 NA
42-Amount of products obtained from balanced chemical equation represents
Actual yield
Practical yield
Theoretical yield
% yield
43-WOF compounds has highest percentage of Oxygen by weight
CH3OH
C2H5OH
HCOOH
H2O
44-Volume occupied by 4.4 g of CO2 at STP is
2.24 dm3
112 cm3
22.4 dm3
1.12 dm3
45-If a ring is made up 6g diamond, then number of atoms present in it are
6.02 x 10^23
3.01 x 10^23
1.5 x 10^23
7.5 x 10^22
46-WOF has least mass
7g of silver
1 gram atom of Nitrogen
3.01 x 10^23 atoms of carbon
1 mole of Neon gas
47-If empirical formula of a compound is CH2 and its molecular mass is 56 amu. What will be its molecular formula
CH2
C3H6
C2H4
C4H8
48-WOF compound have empirical formula, but no molecular formula.
H2O
H2O2
C6H6
NaCl
49-Moles of protons in 20g of SO3
10
40
20
80
50-WOF is a limitation of balanced chemical equation
A-conditions and rate of reactions
B-physical state and mechanism
C-reactants and products and their coefficients
D-both a and b
51-
6Na + Fe2O3 → 3Na2O + 2Fe
For above reaction, if you are provided with 230g of Na and 320g Fe2O3, then limiting reactant is
Na
FeO3
Na2O
None of these
52- 3x10^-21 moles of an amino acid having molecular mass 200 gmol-1, would have molecules
200
1800
300
360000
53-Molecules formula =n x empirical formula, which statement is correct about 'n'
It can never be unity
It may be negative
It can never be zero
Not predictable
54- 11.207 dm3 of methane at STP has ......... Moles of hydrogen atoms.
4
8
2
16
55-The element showing 100% abundance in mass spectrum is
Chlorine
Arsenic
Bromine
Hydrogen
56-Mass of an atom of C is
12/NA g
12 x 1.661 x 10^-24 g
12 amu
All of these
57-WOF isotopes will have maximum deflection in magnetic field during mass spectrometric analysis
C-12
C-14
C-13
Same deflection
58-WOF contains same number of atoms as 12g of Mg
12g Carbon
5g Neon
10g Neon
3g Carbon
59-The sole products of combustion analysis are
CO2 and NH3
CO2 and KOH
H2O and Mg(ClO4)2
CO2 and H2O
60-Styrene has empirical formula CH, and there is 92.2 % C and 7.75% Hydrogen. If molar mass is 104 gmol-1, what will be integral multiple (n) to get molecular formula
2
6
4
8
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