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1a Increased volume of container will decrease the rate of collision between gas molecules and the walls of the container.

1b. Increased temperature will increase the rate of collision because from kinetic theory, temperature is directly proportional to kinetic energy.

1c. Increased molar mass decreases the rate of collision because volume is inversely proportional to pressure.

2 Charles law argues for kinetic molecular theory because volume is directly proportional to temperature which in turns increases the kinetic energy of the gases. this is because of the expansion of air when it is heated, hence gases cannot be static at all times.

3a. N₂ at STP =28g/mol and CH₄ =16g/mol, hence the flask containing N₂ has higher molecular mass(weight) than the flask containing CH₄(methane).

3b. The higher the molar mass and pressure, the denser the gas. Thus the density of the flask containing N₂ is higher than that of CH₄.

3c. Higher speed is correlated with lower masses hence, kinetic energy of CH₄ will be higher than that of N₂

3d. Lighter gases effuses more rapidly hence, CH₄ will effuse through a pin hole leak more rapidly.

4. Effusion is the escape of gas molecules through a tiny hole while diffusion is the distribution of a gas throughout space or throughout another substance.

5. The planet Mercury. This is because, as temperature increases, gases are more likely to approach or obey the ideal-gas law.

6. The constant a, accounts for the attractive forces between the gas molecules. the magnitude of a reflects how strongly the gas molecules attract each other while the constant b is a measure of the actual intrinsic volume occupied by a mole of a gas molecule.