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.
The experiment focuses on investigating the relationship between temperature and the rate of evaporation of three different volatile liquids: methanol, ethanol, and propan-1-ol.
Three identical Petri dishes are labelled A, B, and C, each containing 3.0 cm³ of a different alcohol: methanol (A), ethanol (B), propan-1-ol (C). Each dish is placed inside a temperature-controlled chamber (e.g. warm water bath or incubator) at 60 °C. A digital balance is used to measure mass loss after 5 minutes of heating.
The following data were collected:
| Alcohol | Initial mass / g | Final mass / g | Temperature / °C |
|---|---|---|---|
| Methanol | 2.38 | 0.62 | 60 |
| Ethanol | 2.40 | 1.15 | 60 |
| Propan-1-ol | 2.55 | 1.98 | 60 |
Calculate the average rate of evaporation of methanol in .
Describe the relationship between molecular size and evaporation rate based on the data.
Suggest why propan-1-ol evaporates more slowly than ethanol, despite being under identical conditions.
State the main intermolecular force present in alcohols and explain its origin.
Identify the functional group common to all three alcohols.
Draw a full structural formula of ethanol.
Sketch and label a Maxwell-Boltzmann distribution curve for the ethanol sample at 60 °C. Indicate the activation energy for evaporation and the fraction of particles with enough energy to overcome it.
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.
What volume of carbon dioxide, , can be obtained by reacting of methane, , with of oxygen, ? All volumes are measured at the same temperature and pressure.
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.
A gas has a density of at and . What is its molar mass?
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.
The experiment focuses on investigating the relationship between temperature and the rate of evaporation of three different volatile liquids: methanol, ethanol, and propan-1-ol.
Three identical Petri dishes are labelled A, B, and C, each containing 3.0 cm³ of a different alcohol: methanol (A), ethanol (B), propan-1-ol (C). Each dish is placed inside a temperature-controlled chamber (e.g. warm water bath or incubator) at 60 °C. A digital balance is used to measure mass loss after 5 minutes of heating.
The following data were collected:
| Alcohol | Initial mass / g | Final mass / g | Temperature / °C |
|---|---|---|---|
| Methanol | 2.38 | 0.62 | 60 |
| Ethanol | 2.40 | 1.15 | 60 |
| Propan-1-ol | 2.55 | 1.98 | 60 |
Calculate the average rate of evaporation of methanol in .
Describe the relationship between molecular size and evaporation rate based on the data.
Suggest why propan-1-ol evaporates more slowly than ethanol, despite being under identical conditions.
State the main intermolecular force present in alcohols and explain its origin.
Identify the functional group common to all three alcohols.
Draw a full structural formula of ethanol.
Sketch and label a Maxwell-Boltzmann distribution curve for the ethanol sample at 60 °C. Indicate the activation energy for evaporation and the fraction of particles with enough energy to overcome it.
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.
What volume of carbon dioxide, , can be obtained by reacting of methane, , with of oxygen, ? All volumes are measured at the same temperature and pressure.
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.
A gas has a density of at and . What is its molar mass?