MDCAT Chemistry Online Test With Answers

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MDCAT Chemistry Online Test

Sr. # Questions Answers Choice
1 Deep sea divers breath air under increased pressure, therefore they use a mixture of 96% N<sub>2</sub>and 4% O<sub>2</sub> 96% O<sub>2</sub>and 4% N<sub>2</sub> 94% N<sub>2</sub>and 6% O<sub>2</sub> 94% 0<sub>2</sub>and 6% N<sub>2</sub>
2 What is the mass of 1020molecules of CO2at STP? 7.3 x 10<sup>-3</sup>g 7.9 x 10<sup>-3</sup>g 3.2 x 10<sup>-3</sup>g 4.9 x 10<sup>-3</sup>g
3 What is the numerical value of 'R; (the gas constant) in S.I units? 83143 J/mole/K Avogadro's law 83.143 J/mole/K 8.3143 J/mole/K
4 What is the weight of 10 dm3of CO2at 27°C and 2 atm? 89.3 g 56.1 g 125 g 127 g
5 S.I units for measurements of pressure Pascal mm of Hg atm Torr
6 The attractive forces between molecules of a gas and their sizes can be ignored at high pressure low temperature low temperature and high pressure low pressure and high temperature
7 The ideal gas law holds best under the conditions of high pressure and high temperature low pressure and high temperature low pressure and low temperature high pressure and low temperature
8 At different temperature, the vapour pressure of water is different same low high
9 A term to express the partial pressure of water vapours in a gas is known as vapour pressure aqueous tension partial pressure moisture
10 Which of the following govern the diffusion of gases Dalton's law Avogadro's law Graham's law Newton's law
11 Which gas molecules escape through a hole of molecular dimension this phenomenon is called diffusion mixing effusion flowing of gas
12 Which of the following is not a correct postulate of the kinetic theory of gases the gas molecules are in random motion the collision between the molecules are perfectly elastic the average kinetic energies of different gases are equal at a particular temperature the pressure exerted on the walls of the container is due to intermolecular forces
13 Which gas diffuses more rapidly? O<sub>2</sub> SO<sub>3</sub> NH<sub>3</sub> H<sub>2</sub>
14 For a gas the isotherm is the graph between V and T T and P n and T P and V
15 Which is correct? 1 mm Hg = 1 torr = 1 atm 1 mm Hg = 760 torr = 1 atm 760 mm Hg = 760 torr = 1 atm 760 mm Hg = 1 torr = 1 atm
16 The total pressure exerted by a mixture of gases is the sum of the partial pressure of all the gases present is a statement of Charle's Law Boyle's Law Dalton's Law Graham's Law
17 The rate of diffusion of two gases are inverselly proportional to the square roots of their densities or molecular weights, is a statement of Charle's Law Boyle's Law Graham's Law Dalton's Law
18 At ordinary temperature, the most nearly ideal gases are N<sub>2</sub> He H<sub>2</sub> all these
19 A real gas obeying Vander Waal's equation will resemble ideal gas if Both a and b are large Both a and b are small a is small and b is large a is large and b is small
20 If V1= 5 litters, P1= 2 atm, T1= 273°C, T2= 0°C and V2= ? When P2= 1 atm. 5 lit 10 lit 2.5 lit 12.5 lit
21 Density of a gas is usually expressed in Kg m<sup>3</sup> Kg dm<sup>3</sup> g dm<sup>-3</sup> g cm<sup>-3</sup>
22 The cause of deviation form ideal behaviour is because the actual volume of gas molecules is not negligible there is force of attraction between molecules of a gas both a and b none of these
23 According to Avogadros law 1 mole of gas at S.T.P has a volume of 22.4 dm<sup>3</sup> 24 dm<sup>3</sup> 24000 cm<sup>3</sup> 2m<sup>3</sup>
24 Value of gas constant R is 8.314 J K<sup>-1</sup>mol<sup>-1</sup> 0.082 J K<sup>-1</sup>mol<sup>-1</sup> 273.15 J K<sup>-1</sup>mol<sup>-1</sup> 101325 J K<sup>-1</sup>mol<sup>-1</sup>
25 What is the weight of 10 litres of CO2at 27°C and 2 atm? 89.3 g 36.1 g 125 g 127 g
26 The rate diffusion of H2is 4 times than the of an unknown gas at same temperature and pressure, the molecular mass of unknown gas is 32 16 4 64
27 When a compressed gas is allowed to pass through a nozzle of a jet into a region of low pressure, it produces cooling vaporization fusion expansion
28 Hydrogen has a = 0.245 atm. dm3. mole-2and b = 0.0266 dm3. mole-1SO2gas has a = 6.170 atm. dm3mole-2and b = 0.0564 dm3mole where a and b are Van der Waal's constant H<sub>2</sub>gas deviates more from ideal behaviour tha SO<sub>2</sub> SO<sub>2</sub>gas deviates more form ideal behaviour than H<sub>2</sub> both deviate from ideal behaviour equality both are ideal gases
29 The deviation of a real gas from ideal behaviour is maximum at -10.0<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°C and 50 atm</span> -10<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°C and 2 atm</span> 100<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°C and 2.0 atm</span> 0<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°C and 2 atm</span>
30 Ethene C2H4and N2gases diffuse at the same rate at room temperature. it is due to the reason these are non polar gases their molecular masses are same both are covalent molecules both have multiple bonds
31 The gas which obeys the gas laws at all conditions of temperature and pressure is ideal gas perfect gas real gas noble gas
32 Real gases deviate at low temperature from ideal behaviour due to there is transitional motion of molecule the collissions between the molecules are decreased volume of gas is decreased the inter molecular attractive forces become significant
33 Ar has low critical temperature and pressure due to its small size monatomic molecule low polarizability liquefaction temperature close to room temperature
34 All gases liquefly before reaching at 273<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°K</span> 373<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°K</span> 0 K 73<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°C</span>
35 The highest temperature above which a gas cannot be liquified no matter how much pressure is applied, is called as critical temperature absolute zero liquefaction temperature boiling point
36 The partial pressure of 02in the lungus is 116 torr 159 torr 560 torr 760 torr
37 A mixture of H2, H2 and CH4has total number of 0.51 mole and total pressure of 1 atmosphere. If the mass of H2is 0.8 gram, then its partial pressure is 0.4 atm 0.6 atm 0.776 atm 0.667 atm
38 H2effuses through a porous pot at a rate of 500 cm3per minute at 0°C.The rate of diffusion of O2through the same vessel at 0°C per minute is 500 cm<sup>3</sup> 250 cm<sup>3</sup> 1 dm<sup>3</sup> 125 cm<sup>3</sup>
39 Which pair of the gases doesn't obey Dalton's Law of partial pressures H<sub>2</sub>and O<sub>2</sub> N<sub>2</sub>and O<sub>2</sub> H<sub>2</sub>S and H<sub>2</sub> NH<sub>3</sub>and HCl
40 H2and O2are enclosed in porous vessel. The effusion of these gases will take place like H<sub>2</sub>effuses 4 times the rate of effusion of O<sub>2</sub> O<sub>2</sub>effuses into air 4 times the effusion of H<sub>2</sub> both effuse at same rate H<sub>2</sub>effuses at 8 times the rate of effusion of O<sub>2</sub>
41 Equal masses of CH4and O2are mixed in a 10 dm3container at 25°C. The partial pressures of CH4and O2are in the ratio of 1 : 2 2 : 1 1 : 1 2 : 3
42 The partial pressure of CH4and O2are 500 torr and 100 torr repectively in a 10 dm3vessel at 0°C. The ratio of number of molecules of CH4: O2is 1: 2 5 : 1 5 : 2 2 : 1
43 One dm3of O2at STP has mass 32 g 16 g 4.438 g 1.4383 g
44 The value of R is SI units is 0.0821 dm<sup>3</sup>. atm. J<sup>-1</sup>mole<sup>-1</sup> 62.4 dm<sup>3</sup>torr K<sup>-1</sup>mole<sup>-1</sup> 8.31 dm<sup>3</sup>atm. K<sup>-1</sup>mole<sup>-1</sup> 8.31 JK<sup>-1</sup>mole<sup>-1</sup>
45 If 1 mole of an ideal gas is heated from 273.15 K to 283.15 K at 1 atmospheric pressure, then increase in its energy is 0.082 atm.dm<sup>3</sup> 0.821 atm.dm<sup>3</sup> 8.21 atm.dm<sup>3</sup> 40.6 kJ
46 Density of H2gas at 0°C is 0.09 under 1 atmospheric pressure. The density of O2gas under the same conditions of temperature and pressure is 0.36 1.00 1.44 1.18
47 If a graph is plotted between temperature on x-axis and volume on Y-axis for 1 mole of gas,then we get straight line which cuts the temperature axis at -300<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°C</span> 300 K -273.15 K 273.15<span style="color: rgb(84, 84, 84); font-family: arial, sans-serif; font-size: small;">°C</span>
48 If absolute temperature of a gas is doubled and pressure is reduced to one half, then the volume of the gas will remains unchanged increases unchanged reduces to 1/4 increases 4 times
49 Volume of O2gas at 0°C is 273 cm3, then volume of O2gas at -10°C is 263 cm<sup>3</sup> 163 cm<sup>3</sup> 173 cm<sup>3</sup> 73 cm<sup>3</sup>
50 The gases H2, O2, H2S and SO2diffuse in the order SO<sub>2</sub>&gt;H<sub>2</sub>S&gt;H<sub>2&gt;</sub>O<sub>2</sub> H<sub>2</sub>S&gt;SO<sub>2</sub>&gt;O<sub>2</sub>&gt;H<sub>2</sub> O<sub>2</sub>&gt;SO<sub>2</sub>&gt;H<sub>2</sub>&gt;H<sub>2</sub>S H<sub>2</sub>&gt;O<sub>2</sub>&gt;H<sub>2</sub>S&gt;SO<sub>2</sub>
51 The original volume of a gas at 0° is 273 cm3at constant pressure, its volume at 273°C becomes zero cm<sup>3</sup> 546 cm<sup>3</sup> 446 cm<sup>3</sup> 346 cm<sup>3</sup>
52 Which is the example of diffusion of gases bubbling in soda bottle vapour condensing on a moist surface hot air rising above a candle spreading of smell from a scent bottle
53 The volume of a gas that is occupied by its one mole at STP is called total volume normal volume molar volume atomic volume
54 Equal volume of all gases at same temperature and pressure contain number of molecules different multiples equal in fractions
55 Absolute zero, the lowest temperature on kelvin scale lies at -273<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span> 273<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°</span> -100<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span> 100<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span>
56 According to charles law there will be a change in the volume of a given mass of a gas by 1/273 of its original volume at 0°C if the temperature of the gas is changed by 10<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°</span> 1<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span> 100<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span> 2<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span>
57 The scale of temperature that shows the freezing point of water at 0° is called Fahrenheit Kelvin absolute Celsius
58 The instrument that is used to measure the pressure of a gas is called viscometer photometer barometer stalagmometer
59 Which value is designated as absolute zero or zero of the Kelvin scale? -273.15<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span> -173.15<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span> 273<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: 16px;">°C</span> none of these
60 At constant temperature, volume of given mass of a gas is inversely proportional to pressure on it. This is statement of Charles law Boyle's law Hooks law Grahams law
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