Practice S1.5 Ideal gases with authentic IB Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1A, 1B, 2 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of IB examiners.
A mixture contains equal volumes of hydrogen and oxygen gases at the same temperature and pressure. Which statement is correct?
Which quantity must remain constant for Boyle's law to apply?
A chemistry student heats a gas sample in a sealed container. Initially, the gas occupies a volume of at 290 K and pressure of .
Explain what happens to the pressure of the gas if the temperature increases to 350 K , assuming the volume remains constant.
Calculate the number of moles of gas in the container before heating.
An oxygen cylinder used in hospitals contains oxygen gas at a pressure of and a temperature of . The internal volume of the cylinder is .
State the assumptions made about the particles of an ideal gas.
Calculate the number of moles of oxygen gas in the cylinder.
Calculate the mass of oxygen in the cylinder.
The cylinder is used in an ambulance and left outside in cold weather. Predict and explain the effect of a drop in temperature on the pressure of the gas, assuming constant volume.
Explain why high pressure in a real gas may lead to deviations from ideal gas behavior.
A student collects hydrogen gas produced by the reaction of magnesium with hydrochloric acid. The volume of gas collected is at 298 K and 101 kPa.
Explain why the volume of hydrogen gas collected increases when the temperature rises, assuming pressure remains constant.
Calculate the amount in moles of hydrogen gas collected.
What is the density of carbon dioxide gas at and if its molar mass is ?
A sample of an ideal gas is at and . What volume does it occupy in ?
A student collects a gas sample in a syringe after a reaction between magnesium and hydrochloric acid. The volume of gas collected is at and .
Convert the gas volume to for use in calculations.
Use the ideal gas equation to calculate the amount in moles of gas collected.
Magnesium reacts with excess according to:
Determine the mass of magnesium that would have been used to produce this amount of gas.
State one assumption made when using the ideal gas law in this experiment.
Which sample contains the fewest moles of HCl?
Molar volume of an ideal gas at STP .
Which of the following assumptions in the kinetic molecular theory is least valid for real gases at low temperature and high pressure?
Practice S1.5 Ideal gases with authentic IB Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1A, 1B, 2 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of IB examiners.
A mixture contains equal volumes of hydrogen and oxygen gases at the same temperature and pressure. Which statement is correct?
Which quantity must remain constant for Boyle's law to apply?
A chemistry student heats a gas sample in a sealed container. Initially, the gas occupies a volume of at 290 K and pressure of .
Explain what happens to the pressure of the gas if the temperature increases to 350 K , assuming the volume remains constant.
Calculate the number of moles of gas in the container before heating.
An oxygen cylinder used in hospitals contains oxygen gas at a pressure of and a temperature of . The internal volume of the cylinder is .
State the assumptions made about the particles of an ideal gas.
Calculate the number of moles of oxygen gas in the cylinder.
Calculate the mass of oxygen in the cylinder.
The cylinder is used in an ambulance and left outside in cold weather. Predict and explain the effect of a drop in temperature on the pressure of the gas, assuming constant volume.
Explain why high pressure in a real gas may lead to deviations from ideal gas behavior.
A student collects hydrogen gas produced by the reaction of magnesium with hydrochloric acid. The volume of gas collected is at 298 K and 101 kPa.
Explain why the volume of hydrogen gas collected increases when the temperature rises, assuming pressure remains constant.
Calculate the amount in moles of hydrogen gas collected.
What is the density of carbon dioxide gas at and if its molar mass is ?
A sample of an ideal gas is at and . What volume does it occupy in ?
A student collects a gas sample in a syringe after a reaction between magnesium and hydrochloric acid. The volume of gas collected is at and .
Convert the gas volume to for use in calculations.
Use the ideal gas equation to calculate the amount in moles of gas collected.
Magnesium reacts with excess according to:
Determine the mass of magnesium that would have been used to produce this amount of gas.
State one assumption made when using the ideal gas law in this experiment.
Which sample contains the fewest moles of HCl?
Molar volume of an ideal gas at STP .
Which of the following assumptions in the kinetic molecular theory is least valid for real gases at low temperature and high pressure?