Partial Pressure MCQ

Test your knowledge with important Partial Pressure MCQ and their applications. These MCQs are beneficial for competitive exams too. Explore 30 + more Partial Pressure MCQs at Bissoy

• 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 5.05 moles of the gas was in it?
  ক

  896.20 torr

  খ

  796.20 torr

  গ

  596.20 torr

  ঘ

  696.20 torr
• In an experiment,the barometric pressure of gas is 1.043 atm, Some H2 was collected over water at 27.0°C. What is the partial pressure of the dry H2 in the container?
  ক

  0.1021 atm

  খ

  102.1 atm

  গ

  10.21 atm

  ঘ

  1.021 atm
• Which of the following statements about partial pressure are correct? Statement 1: The partial pressure of each gas in a mixture is not proportional to its mole fraction.. Statement 2: The partial pressure of each gas is the product of the total pressure and the mole fraction of that gas.
  ক

  True, False

  খ

  True, True

  গ

  False, True

  ঘ

  False, False
• What is the limitation of Dalton’s law?
  ক

  It implies only for real gases at low pressure

  খ

  It implies only for real gases at high pressure

  গ

  It implies only for real gases at low concentration

  ঘ

  It implies only for real gases at high concentration
• Does partial pressure depend on temperature?
  ক

  True

  খ

  False
• Which of the following component is constant in Boyle’s law?
  ক

  Concentration

  খ

  Pressure

  গ

  Temperature

  ঘ

  Volume
• What is r value in pV= nRT?
  ক

  0.8314 J/mol•K

  খ

  831.4 J/mol•K

  গ

  83.14 J/mol•K

  ঘ

  8.314 J/mol•K
• What is partial pressure of water vapor?
  ক

  23.8 mm Hg

  খ

  230.8 mm Hg

  গ

  2.38 mm Hg

  ঘ

  0.238 mm Hg
• What is the use of partial pressure?
  ক

  To predict the movement of gases

  খ

  To predict the concentration change

  গ

  To predict the pressure change

  ঘ

  To predict the mole fraction
• How to calculate partial pressure?
  ক

  Sum of the pressures of each individual gas

  খ

  Total pressure multiplied by the mole fraction of that gas

  গ

  Sum of the mole fraction of each individual gas

  ঘ

  Total concentration multiplied by the mole fraction of that gas