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WorksheetsStates of Matter: Gas
Total questions: 8
Worksheet time: 4mins
Choose the INCORRECT statement about the assumptions of the kinetic molecular theory.
The collision between gas molecules is elastic.
The volume of gas is negligible compared to the volume of container.
At constant temperature, each molecule has the same velocity.
Gas molecules move randomly and continuously.
“At constant temperature and pressure the volume of a gas is directly proportional to the number of moles of the gas”
The law describes the above statement is
Charles’ law
Avogadro’s law
Boyle’s law
Ideal Gas law
Gas behaves almost ideally at very low pressure. As the pressure is lower.
The gas molecules are far apart from each other.
Intermolecular forces become weaker.
Volume of the gas decreases.
It obeys kinetic molecular theory.
Which of the following is NOT TRUE?
Viscosity increases as temperature increases.
Viscosity arises because of cohesive forces within the liquid molecules.
Viscosity increase with stronger intermolecular forces.
Liquid with low viscosity can flow freely.
The following factors affecting the vapour pressure of a liquid EXCEPT
volume of liquid.
temperature.
molecular size of liquid.
relative molecular mass of liquid.
According to Boyle’s Law, the relationship between pressure and volume of a fixed amount of gas at constant temperature is:
Directly proportional
Inversely proportional
Remains constant regardless of changes
Independent of each other
When plotting the graph of V vs T (in °C) for a fixed amount of gas at constant pressure, the line intercepts the x-axis at –273 °C. What does this suggest?
Gas molecules stop moving completely at 0 °C.
Pressure of the gas becomes zero at room temperature.
Volume of a gas theoretically becomes zero at absolute zero.
Real gases cannot exist above –273 °C.
Two identical flasks at the same temperature and pressure are filled separately with 2 g of hydrogen (H₂) and 32 g of oxygen (O₂). Which statement best explains why the pressure inside both flasks is the same?
As both samples are kept at constant volume, any change in pressure is prevented according to Boyle’s Law.
The lighter hydrogen molecules move faster than oxygen molecules, but their higher velocity balances the lower molecular mass, producing the same pressure. (Kinetic Molecular Theory)
Both flasks contain the same amount of molecules, because each sample is 1 mol of gas. (Avogadro’s Law)
Because temperature is the same, the gases expand equally and thus exert the same pressure, as explained by Charles’s Law.
