Posted inunclassified Chemistry: Behavior of Gases Posted by By Agodirin October 17, 2024No Comments Report a question What's wrong with this question? You cannot submit an empty report. Please add some details. 3 1234567891011121314151617181920212223242526272829303132333435363738394041424344454647484950 Created by Agodirin Behavior of Gases 1 / 50 1. gas1_Which of the following is correct about an inflated air-filled balloon placed in hot water A) the balloon will grow in size because the increased temperature increase the kinetic energy of the gas molecules B) the balloon will shrink because the van dar waal forces between the gas molecules increase C) the balloon will shrink because the gas molcules will lose kinetic energy to the warm water D) the balloon will grow bigger because of condensation Heating the air inside the balloon increases the kinetic energy of the gas molecules, causing the balloon to expand 2 / 50 2. gas1_Which of the following is not true about the Kinetic theory of a fixed mass of gas A) increase in temperature causes increase in kinetic energy B) an increase in the temperature increases the frequency of collision with the walls C) the gas pressure is due to continuous bombarbment of the wall of the container by gas molecules D) increase in temperature causes reduction in the pressure According to kinetic theory, increasing temperature increases pressure, as it increases the kinetic energy and frequency of collisions with the walls of the container. 3 / 50 3. gas1_The basic assumption in the kinetic theory of gases that the collisions of the gaseous molecules are perfectly elastic implies that the? A) gaseous molecules can occupy any available space B) gases can be compressed C) forces of attraction and repulsion are in equilibrium D) gaseous molecules will continue their motion indefinitely The basic assumption in the kinetic theory of gases that the collisions of the gaseous molecules are perfectly elastic implies that the gaseous molecules will continue their motion indefinitely. In a perfectly elastic collision, there is no loss of kinetic energy, so the molecules continue moving after colliding with each other or with the walls of the container. This assumption helps explain the behavior of gases, such as their ability to fill any available space and their compressibility. However, the key point regarding elastic collisions is the indefinite continuation of motion 4 / 50 4. gas1_A sample of a gas occupies a voluem of 0.6dm3 at temperature of 430K and at atmospheric pressure. What will be the voluem of the gas at 430K and at 507mmhg [atm pressure=760mmhg] A) 0.5dm3 B) 0.3dm3 C) 0.7dm3 D) 0.9dm3 Using P1VI= P2V2 at constant temperature: V2=(760mmHg)×(0.6dm3)/507mmhg≈0.9dm3 5 / 50 5. gas1_the value of absolute zero temprature is A) -273 B) 300K C) 273K D) 0K Absolute zero is defined as 0 K, which corresponds to -273.15°C. 6 / 50 6. gas1_which of the following correctly represents boyle's law, where K is constant , V is volume and P is pressure A) V=k x P B) V= k x 2P C) V=k/P D) V=p/k V = k/P Explanation: This equation shows that volume (V) is inversely proportional to pressure (P).... 7 / 50 7. gas1_When air is compressed? A) its temperature increases B) it solidifies C) its temperature decreases D) its density decreases When air is compressed, its temperature increases. This is due to the principles of thermodynamics. When a gas is compressed, the volume available reduces, the molecules are forced closer together, which increases the frequency and intensity of collisions among them, leading to an increase in temperature. This phenomenon is often observed in processes such as in bicycle pumps or internal combustion engines 8 / 50 8. gas1_Which of the following is not a physical property of gases A) low boiling point B) ability to expand C) high density D) ability to condense Gases generally have low densities compared to solids and liquids, as their molecules are far apart. "Low boiling point," "ability to condense," and "ability to expand" are all physical properties of gases. 9 / 50 9. gas1_A gas placed in a container collides with the wall of the container at a frequency 'F'. If the volume of the container reduces by half and the temperature remains constant. Which of the following will occur A) the frequency of collision will be F/2 B) the frequency of collition will be 2F C) the frequency of collision will be F squared D) the gas will stop colliding with the wall Reducing the volume increases the frequency of collisions between gas molecules and the walls, thus doubling the frequency of collisions. 10 / 50 10. gas1_To what temperature must a gas at 273K be heated in order to double its volume and pressure A) 546K B) 819K C) 1092K D) 298K Given the initial temperature T1=273K, and knowing we want to double both the volume (V2=2V1) and the pressure (P2=2P1), we can use the combined gas law: P1V1/T1=P2V2/T2. Plugging in the values: P1V1/273K=(2P1)⋅(2V1)/T2. We simplify to: 1273=4T2. Solving for T2: T2=4×273=1092K 11 / 50 11. gas1_A substance has boiling point of 4 degree celcius. If the room temperature is 25 degree celcius , the substance is likelty to be A) solid B) gas C) liquid D) mixture of solid and liquid Since the room temperature is 25 degrees Celsius, which is higher than the substance's boiling point of 4 degrees Celsius, the substance is likely to be in the gas state at room temperature 12 / 50 12. gas1_Which of the following is the boyle's law A) the temperature of a given mass of gas is directly proportional to the volume at a constant pressure B) the volume of a given mass of gas is a multiple of the pressure at a constant temperature C) the volume of a given mass of gas is inversely proportional to the pressure at a constant temperature D) the volume of a given mass of gas is directly proportional to the volume at a constant temperature Boyle's Law states that, for a fixed amount of gas at constant temperature, the volume is inversely proportional to pressure. 13 / 50 13. gas1_Which of the following correctly represents the mathematical equation for the general gas equation A) VT/P=k B) PV/T=k C) PT/V=k D) P/VT=k PV/T = k. Explanation: This is the correct form of the ideal gas law represented in a rearranged format, indicating that pressure times volume divided by temperature equals a constant. 14 / 50 14. gas1_the value of standard temperature and pressure (S.T.P) are A) 273K and 700mmhg B) 100K and 760mmhg C) 273K and 760mmhg D) zero degree celcius and 273mmhg Standard Temperature and Pressure (S.T.P) is defined as 273K (0°C) and 760 mmHg. 15 / 50 15. gas1_A gas exerts pressure on its container because? A) the molecules of a gas collide with the walls of the container B) of the mass of the molecules of the gas C) some of the molecules are moving faster than others D) of the collisions of the molecules with each other Gas pressure is created by the collisions of gas molecules with the walls of their container. As gas molecules move randomly and collide with the walls, they exert force on those walls, resulting in pressure 16 / 50 16. gas1_A mass of gas has Pressure P1 and volume V1 . If the Pressure of the container is increased. Which of the following will occur A) the volume will remain V1 B) the volume in reduce C) the volume will increase D) the volume will double According to Boyle's Law, at constant temperature, the pressure and volume of a gas are inversely related. If pressure increases, volume must decrease 17 / 50 17. gas1_which of the following characteristics determines the direction of diffusion or flow of gases A) temperature B) volume C) pressure D) light Gases diffuse from areas of high pressure to areas of low pressure. This is a fundamental principle of gas behavior. 18 / 50 18. gas1_the ability of gases to change to liquid under high pressure and low temperature is A) sublimation B) condensation C) evaporation D) expansion Condensation is the process by which a gas transforms into a liquid, typically occurring when the gas is subjected to high pressure and/or low temperature. 19 / 50 19. gas1_which of the following is not correct about absolute zero temperature point A) there is rapid motion of particles at absolute zero temperature B) the value of absolute zero temperature is -273 C) the kinetic energy is zero at the absolute zero temperature D) the unit of absolute zero temperature is kelvin At absolute zero, particle motion theoretically ceases, and kinetic energy is at a minimum. 20 / 50 20. gas1_A car tyre was inflated to pressure of P. after driving a long distance on a sunny day ,what will happen to the pressure A) it will increase B) it will not change C) it will fluctuate between reducing and the initial pressure D) it will reduce As the temperature of the air inside the tire increases due to heat from the environment, the pressure will also increase (Gay-Lussac's Law) 21 / 50 21. gas1_which of the following is charles' law A) the volume of a given mass of gas is inversely proportional to its pressure at constant temperature B) the volume of a given mass of gas is inversely proportional to its temperature at a constant pressure C) the volume of a given mass of gas is directly proportional to its pressure at constant temperature D) the volume of a given mass of gas is directly proportional to the absolute temperature at a constant pressure Charles' Law states that volume increases with an increase in temperature, provided pressure is constant. 22 / 50 22. gas1_An ideal gas with Pressure P1 and Volume P1 is subjected to pressure P2 at constant temperature. Which of the following is correct about the behavior of the gas A) P1V1 will be equalt 2P1V1 B) P1V1 will be equal to P2V2 C) P1V1 will be equal to 1/2P1V2 D) P1V1 will be equal to P1V1/2 This is a direct application of Boyle's Law, which states that P1V1=P2V2 when temperature is constant 23 / 50 23. gas1_A gas measures 1dm3 at a temperature of 27 oC and 300mmhg. To what temperature must the gas be heated when the pressure rises to 480mmhg for the volume to remain unchanged A) 300oC B) 207oC C) 480oC D) 273oC Initial conditions: Volume, V=1dm3, Temperature, T1=27∘C=300K, Pressure, P1=300mmHg. Final conditions: Pressure, P2=480mmHg and volume remains constant. Using the combined gas law: P1/T1=P2/T2, T2=P2×T1P1, T2=480×300/300, T2=480K. to Celsius = 480-273=207oC 24 / 50 24. gas1_1 atmosphere pressure is equal to A) 273mmhg B) 700mmhg C) 10mmhg D) 760mmgh Standard atmospheric pressure is defined as 760 mmHg. 25 / 50 25. gas1_Which of the following is NOT one of the well defined states in which matter occur A) volatile B) gas C) liquid D) solid Matter exists in three primary states: solid, liquid, and gas. These states are well-defined based on the arrangement of molecules, energy levels, and physical properties. "Volatile" is not a state of matter but rather describes a substance's tendency to vaporize 26 / 50 26. gas1_Which of the following is not correct about the kinetic theory of gases A) During collision the molecules of gases have strong attractive forces pulling them together B) the collision between gas molecules is perfectly elastic: meaning no energy is lost C) the average kinetic energy of the gas molecules is directly proportional to the temperature D) the molecules of the gas collide with each other and with the wall of the container The kinetic theory of gases assumes that there are negligible attractive forces between gas molecules, allowing them to move freely and collide elastically without strong interactions. 27 / 50 27. gas1_The temperature of a gas is 57 degree Celsius at what temperature will its original volume be halved while the pressure is tripled A) 328OC B) 222OC C) 342OC D) 162OC 222 cm³. Explanation: Using the combined gas law (P1V1/T1= P2V2/T2), we can find the new volume at standard pressure while keeping temperature constant. (remember that to use the formula you convert the temperature to Kelvin scale) 28 / 50 28. gas1_The pressure a gas exerts when it is alone in a container is called its A) similar pressure B) partial pressure C) combined pressure D) absolute pressure That would be called its partial pressure. This term is particularly useful when dealing with mixtures of gases, as it helps to understand the contribution of each individual gas to the total pressure. 29 / 50 29. gas1_the mathematical equation for charles' low is A) V= k x 2T B) V=p/T C) V=k x T D) V=k/T V = k × T. Explanation: This equation shows that volume (V) is directly proportional to temperature (T) at constant pressure 30 / 50 30. gas1_convert temperature of 280K to Celcius A) 14C B) 7C C) 273C D) 297C Using the standard formula relationship between kelvin and celsius (K=273+ Celsius) °C=K−273°C=K−273. So, 280K−273=7°C280K−273=7°C 31 / 50 31. gas1_A gas sample with initial volume of 3.25dm3 is heated and allowed to expand to 9.75dm3 at constant pressure . What is the ratio of the final absolute temperature to the initial absolute temperature A) 1;3 B) 3;1 C) 3;2 D) 2;3 Since volume increases, absolute temperature must also increase proportionally if pressure is constant 32 / 50 32. gas1_The molecules of gas have different kinds of motion, which of the following is not one of them A) rotatory B) static C) translatory D) vibratory Gas molecules are always in motion, exhibiting translational, rotational, and vibrational motion. "Static" suggests no movement, which does not apply to gases. 33 / 50 33. gas1_A mass of gas occupies 100cm3 at 1.0x 105Nm-2, what will be the volume of the gass at 0.5x 105Nm-2. If the temperature remains constant A) 100cm3 B) 300cm3 C) 50cm3 D) 200cm3 Initial Volume V1=100 cm3. Initial Pressure P1=1.0×105 Nm-2 Final Pressure P2=0.5×105 Nm−2. Using Boyle's Law, which states that P1V1=P2V2 (at constant temperature):V2=P1V1/P2. Will result in 200cm3 34 / 50 34. gas1_Zero degree celcius is equal to A) 300K B) 100K C) 760K D) 273K This is the same conversion as above; zero degrees Celsius converts to 273 Kelvin. 35 / 50 35. gas1_which of the following is not correct A) the volume of gas increases as the temperature increases B) the direction of gas flow or diffusion is from high pressure to low pressure C) the volume of gas increases as the pressure increases D) the volume of gas reduces as the temperature reduces the volume of gas increases as the pressure increases . · Explanation: This statement is incorrect according to Boyle's Law, which states that the volume of a gas decreases as pressure increases (at constant temperature) 36 / 50 36. gas1_which of the following is not correct about an air-filled balloon placed in hot water A) the gas molecules will move faster B) the kinetic energy of the gas molecules will increase C) the balloon will increase in size because of condensation D) the gas molecules will collide more frequently with the wall of the balloon Heating the gas increases the kinetic energy of the gas molecules, leading to expansion, not condensation. Condensation typically occurs when gas cools and changes to liquid 37 / 50 37. gas1_Which of the following is not correct about the kinetic theory of gases A) Gas consist of many tiny molecules moving randomly in straight line B) there is no attractive forces between the molecule of gas C) the molecules of the gas collide with one another but not with the wall of the container D) the volume of the gas is small compared to the volume it occupies the molecules of the gas collide with one another but not with the wall of the container Explanation: This statement is incorrect because, according to the kinetic theory of gases, gas molecules do collide with each other and also with the walls of their container. These collisions are essential for explaining pressure 38 / 50 38. gas1_An oxide XO2 has a vapour density of 32. What is the atomic mass of X A) 32 B) 14 C) 12 D) 20 To find the atomic mass of element X in the oxide XO2 with a given vapor density, we can use the relationship between vapor density and molar mass. Vapor Density (VD) Formula:=Molar Mass/2. Given that the vapor density is 32, we can calculate the molar mass: Molar Mass=2×Vapor Density=2×32=64 g/mol. Molar Mass of XO2. Molar Mass of XO2=Atomic Mass of X+2×Atomic Mass of O The atomic mass of oxygen (O) is approximately 16 g/mol. Therefore: Molar Mass of XO2=Atomic Mass of X+2×16 =Atomic Mass of X+2×16=Atomic Mass of X+32. Since we know the molar mass of XO2XO2 is 64 g/mol, we can set up the equation: Atomic Mass of X+32=64Atomic Mass of X+32=64. Hence atomic mass of X= 64-32 39 / 50 39. gas1_273K is equal to A) 100 degree celcius B) zero degree celcuis C) 300 degree celcius D) 30 degree celcius 0°C is equivalent to 273K based on the conversion formula. 40 / 50 40. gas1_The ratio of initial to final pressure of a gas is 1:1.5 calulate the final volume if the initial volume was 300cm3 A) 150cm3 B) 200cm3 C) 400cm3 D) 350cm3 Using Boyle's Law, if the pressure increases by a factor of 1.5, the volume will decrease to 300/1.5=200 cm³... 41 / 50 41. gas1_A substance that has boiliing point below room temperature is A) gas B) solid C) soft D) liquid Substances with boiling points below room temperature (approximately 20-25°C) will exist as gases at standard atmospheric pressure. For example, substances like propane and butane are gases at room temperature. 42 / 50 42. gas1_Which of the following does not explain why an increase in temperature of a gas of fixed volume results in increase pressure A) increase temperature cause increase motion of the gas molecules B) increase temperature cause increase condensation of the gas molecule on the container wall C) increase temperature cause increase bombardment of the wall of the contain by the gas molecules D) increase temperature cause increase kinetic energy of gas molecules Increased temperature leads to increased energy and movement, not condensation, which would occur at lower temperatures. 43 / 50 43. gas1_What are the two variables that determine th volume of a fixed mass of gas A) temperature and pressure B) type of gas and nature of container C) gravity and force D) container and time of the day According to gas laws, the volume of a gas is affected by its temperature and pressure. 44 / 50 44. gas1_Convert temperature of 27 degree celcius to Kelvin A) 300K B) 273K C) 263K D) 327K Using the standard formula relationship between kelvin and celsius (K=273+ Celsius) To convert Celsius to Kelvin, you add 273.15 to the Celsius temperature: 27+273.15=300.15 K≈300 45 / 50 45. gas1_which of the following is not correct. A) When the temperature of a gas increases the volume increases B) when the temperature of a gas increases the pressure reduces C) The relationship between volume and pressure of gas was described by Boyle D) The relationship between volume and temperature of gas was described by Charlse According to Gay-Lussac's Law, if volume is constant and temperature increases, pressure increases 46 / 50 46. gas1_What is the teperature of a given mass of gas initially at 0 degree celsius and 9 atmosphere, If the pressure reduces to 3 atmosphere at constant volume A) 819K B) 273K C) 182K D) 91K Using the combined gas law: P1/T1=P2/T2. T2=P2×T1P1, T2=3×2739, T2=91K 47 / 50 47. gas1_A certain mass of gas occupies 330cm3 at 27 degree celsius and 9.0x 104 Nm-2. Calculate its volume at S.T.P (Standard pressure= 1.0 x105 Nm-3 A) 240cm3 B) 150cm3 C) 380cm3 D) 270cm3 270 cm³. Explanation: Using the combined gas law (P1V1/T1= P2V2/T2), we can find the new volume at standard pressure while keeping temperature constant. (remember that to use the formula you convert the temperature to Kelvin scale) 48 / 50 48. gas1_Which of the following statements is NOT correct? A) The average kinetic energy of a gas is directly proportional to its temperature B) At constant temperature, the volume of a gas increases as the pressure increases C) The pressure of a gas is inversely proportional to the density D) The temperature of a gas is directly proportional to its volume At constant temperature, the volume of a gas increases as the pressure increases. Explanation: This statement is incorrect; at constant temperature, an increase in pressure results in a decrease in volume (Boyle's Law). 49 / 50 49. gas1_Which of the following statements is correct about intermolecular distances and cohesive forces between gas respectively? They are A) constant and negligible respectively B) both negligible C) large and negligible respectively D) both large Large and negligible. Explanation: Intermolecular Distances: In gases, the molecules are far apart compared to liquids and solids, resulting in large intermolecular distances. Cohesive Forces: The cohesive forces (attractive forces between molecules) in gases are negligible because the distance between the molecules is so great that these forces have minimal effect on the behavior of the gas. Thus, gases have large intermolecular distances and negligible cohesive forces 50 / 50 50. gas1_The volume of a fixe mass of gas measured at atmospheric pressure nad 27 degree celsius is 3.0dm3. Calculate the volume at 127 degree celsius A) 2dm3 B) 5dm3 C) 4dm3 D) 3.5dm3 Using Charles' Law, convert temperatures to Kelvin and find the new volume using the direct proportionality. 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