Q.1
##### What is the limitation of Dalton’s law?
• a) It implies only for real gases at low pressure
• b) It implies only for real gases at high pressure
• c) It implies only for real gases at low concentration
• d) It implies only for real gases at high concentration
Q.2
##### Which of the following statements about partial pressure are correct?
• a) True, False
• b) True, True
• c) False, True
• d) False, False
Q.3
##### How to calculate partial pressure?
• a) Sum of the pressures of each individual gas
• b) Total pressure multiplied by the mole fraction of that gas
• c) Sum of the mole fraction of each individual gas
• d) Total concentration multiplied by the mole fraction of that gas
Q.4
##### What is the use of partial pressure?
• a) To predict the movement of gases
• b) To predict the concentration change
• c) To predict the pressure change
• d) To predict the mole fraction
Q.5
##### What is partial pressure of water vapor?
• a) 23.8 mm Hg
• b) 230.8 mm Hg
• c) 2.38 mm Hg
• d) 0.238 mm Hg
Q.6
##### What is r value in pV= nRT?
• a) 0.8314 J/mol•K
• b) 831.4 J/mol•K
• c) 83.14 J/mol•K
• d) 8.314 J/mol•K
Q.7
##### Which of the following component is constant in Boyle’s law?
• a) Concentration
• b) Pressure
• c) Temperature
• d) Volume
Q.8
• a) True
• b) False
Q.9
##### In an experiment,the barometric pressure of gas is 1.atm, Some H2 was collected over water at 27.0°C. What is the partial pressure of the dry H2 in the container?
• a) 0.1021 atm
• b) 102.1 atm
• c) 10.21 atm
• d) 1.021 atm
Q.10
##### The pressure of a 2.74moles of a gas in a container was 432.0 torr. What would the pressure inside the container be if 5.moles of the gas was in it?
• a) 896.20 torr
• b) 796.20 torr
• c) 596.20 torr
• d) 696.20 torr