MDCAT Chemistry Online Test With Answers

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MDCAT Chemistry Online Test

Sr. # Questions Answers Choice
1 An ideal gas expands according to PV=constant. On expansion, the temperature of gas will rise will drop cannot be determined because the exteral pressure is not known will remain same
2 The density of neon will be highest at STP 0°C, 2 atm 273°C, 1 atm 273°C, 2 atm
3 If a gas expands at constant temperature The pressure decreases The Kinetic energy of the molecules remains the same The kinetic energy of the molecules decreases The number of molecules of the gas increase
4 What are the conditions under which the relation between volume (V) and number of moles (n) of gas is plotted? (Pressure; T-temperature) constant P and T constant P and V constant T and V constant n and v
5 An ideal gas, obeying Kinetic theory of gases cannot be liquified, because its critical temperature is above 0°C its molecules are relatively small in size It solidifies before becoming a liquid Forces acting between its molecules are negligible
6 If temperature is 73K and volume is 146 cm3 then calculate the value of K=V/T 5 4 3 2
7 The volume of given mass of gas is directly proportional to absolute temperature when pressure is kept constant this is called Boyle's law Charles's law Graham's law Dalton's law
8 Which type of motion is exhibited by gases? Vibrational Transitional Rotational All of them
9 For an ideal gas, number of mole in terms of its pressure P, temperature T and gas constant is PT/R PRT PV/RT RT/P
10 Helium atom is two times heavier than a hydrogen molecule. At 298 K, the average kinetic energy of a helium atom is same as that of a hydrogen molecule half that of a hydrogen molecule two times that of a hydrogen molecule four times that of hydrogen molecule
11 If increase in temperature and volume of an ideal gas is two times, then the initial pressure P changes to 4P P 2P 3P
12 Styrene has empirical formula CH, and there is 92.2%C and 7.75% hydrogen. If molar mass is 104g mol¯, what will be integral multiple (n) to get molecular formula: 2 4 6 8
13 The sole produets of combustion analysis are CO2 and NH3 H2O and Mg(CIO4)2 CO2 and KOH CO2 and H2O
14 6Na+ Fe2O3 -------- 3 Na2O+2Fe For above reaction, if you are provided with 230g Na and 320g Fe2O3, then limiting reactant is , Na Na2O Fe2O3 none of these
15 Which of the following is a limitation of balanced chemical equation Conditions and rate of reactions Physical state and mechanism Reactants and products and their coefficients Both (a) and (b)
16 Moles of protons in 20g of SO3 10 20 40 80
17 Which of the following compound have empirical formula, but no molecular formula H20 C6H6 H<sub>2</sub>O<sub>2</sub> NaCl
18 If empirical formula of a compound is CH2 and its molecular mass is 56amu. What will beits molecular formula CH2 C3H6 C2H4 C4H8
19 Atoms having same mass number but different atomic numbers are called. Isotopes isobars Isotones isomers
20 Naturally occurring isotopes of silver are ,Two , Four , Forty seven , sixteen
21 How many isotopes are present in palladium Two Four Six nine
22 Which of the following is pure substance Distilled water , Sea water , NaCl (aq) Brass
23 Haemoglobin molecule is how many times heavier than helium atom 68000 times 17000 times ,34000 times , 1700 times
24 The best concentration unit used for K⁺ ions present in potable water is ppm Mole fraction Molarity Molality
25 The molarity of 2% W/V NaOH solution is 2 0.25 0.05 0.5
26 In s solution 7.8 g of benzene ( C6H6 ) and 46g of toluene (C6H5CH3) is present. The mole fraction of toluene is 1/3 1/5 2/3 5/6
27 The number of moles of CO2 which contain 16g of oxygen 0.25 1.00 1.50 0.50
28 The largest number of molecules are present in 3.6 g of H2O 4.6 g of C2H5OH 2.8 g of CO 5.4 g of N2O5
29 When we dissolve 15.8 g of KMnO4 in 1000g of H20. The solution is , 0.1 M 0.1 M 0.2 M 0.2 M
30 How many grams of NaOH are present in 250 cm3 of its 0.2M solution ,4 g , 0.4 g , 10 g , 2 g
31 When liquid solute is dissolved in liquid solvent, then the best unit of concentration is? % W/W % W/V % V/V %V/W
32
250cm of 0.2 molar potassium sulphate solution is mixed with 250cm of 0.2 molar KCI solution. The molar concentration of K ions is:
 0.2 molar 0.25 molar 0.3 molar 0.35 molar
33 Combustion analysis is performed for the determination of Molar mass of the compound Empirical formula of the compound Structural formula of the substance Mass of halogens present in organic compounds
34 The height of the peak in the mass spectrum shows Number of isotopes Relative abundance Mass number Number of protons
35 Molecular ions are produced in mass spectrometer. Which type of molecular ion formed more abundantly. Negatively charged H⁺ ions Positively charged equal positive and negative ions
36 During combustion analysis, which one is used for absorbing carbon dioxide: 50% KOH 5% KOH Mg(ClO4)2 Silica gel
37 Which of the following contains I 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
38 Gram atoms of hydrogen in 5.5 g H2 5.50 2.25 5.45 2.20
39 Number of moles present in 0.6 gram of silica is (Atomic mass Si = 28, O=16) 0.01 mole 0.064 mole 0.044 mole 0.054 mole
40 5604 cm3 of H2 gas at STP contains atoms of hydrogen 6.02×10 (23) 2.6x10(22) 3.01x10(23) 1. 50x 10(23)
41
Mg(s) + 2HCI(aq). ------------ MgCl2(aq)+ H2(g)
Given that; Mg=21g and HCI=21g, the excess reactant is
 Mg HCI Both are in stoichiometric amounts None of these
42 One mole of SO2 contains 6.022 x 10(23) atoms of oxygen 6.022x 10 ê23 atoms of sulfur 18.1x 10 (23) molecules of SO2 4 g molecule of SO2
43 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: 6.02x10ê23/1.0x10ê-6 1.0x 10ê-6 x 6.02x 10ê23 1.0x10ê-6 x 6.02×10ê23/20.2 1.0x10ê-6 x 6.02x10ê23/9.65x10ê-1
44 1 gram formula refers to Amount in grams equivalent to 1 mole of a atom Amount in grams equivalent to 1 mole of a covalent compound Amount in grams equivalent to 1 mole of a ionic compound Amount in grams equivalent to 1 mole of an ion
45 Number of H+ ions when 0.1 mole of sulfuric acid is completely ionized in water 4x6.022x10ê23 1×6.022x10ê23 2x6.022 x10ê23 2x6.022x10ê22
46 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
47 The stoichiometric calculations for a chemical reaction results in Actual yield Percentage yield Theoretical yield Selectivity
48 Mass spectrometry is used to determine the Number of isotopes of an element Relative abundance of isotopes Relative isotopic masses All of these
49 Inside every fluorescent lamp there is present a: Gas Plasma Liquid Solid
50 Most of the universe consists of the matter in : Gaseous state Liquid state Plazma state Solid state
51 The basic distinction between solids, liquids and gases lies in difference between. Strength of the bonds Size of molecules space which the molecules occupy All of above
52 At 100 atm, CH4 develops: Ideal attitude Non-ideal attitude Serious attitude Laughing attitude
53 The gas which obey's the gas laws at all conditions of temperature and pressure is called: Perfect gas Super gas Ideal gas Real gas
54 Absolute zero is equal to: -273.15K -273.15<sup>o</sup>C -237.15K -273 <sup>o</sup>C
55 The critical temperature of NH3 is greater than CO2 due to its: Greater polarity Stable polarity Lesser polarity None of above
56 When a compressed gas is allowed to expand into a region of low pressure, it produce: Vapours Cooling effect Heating effect None of above
57 During sudden expansion of a gas energy is needed to overcome the intermolecular: Vibrations Attractions Repulsions All of above
58 The non polar gases of low polarizability have a very: Low critical temperature Stable critical temperature High critical temperature
59 The value of critical temperature of a gas depends upon its: Size Intermolecular forces in it Shape All of above
60 An ideal gas cannot be liquefied because: It solidify before becoming a liquid Its critical temperature is always above 0<sup>o</sup>C It is molecule are relatively smaller in size. Forces operative between its molecules are negligible
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