Raising solvent temperature causes solvent-solute collisions to become

raising solvent temperature causes solvent-solute collision to become more rapid in the sense that the collision gain more kinetic energy.

Explanation:

When the temperature of a solvent is increased, kinetic energy (motion) is increased. The rate of collision of solvent to solute increases as temperature rises. Solvent to solute collision move rapidly with force when temperature is increased.

Increase in temperature also increase solubility of solute in solvent. As the solvent temperature is increased, kinetic energy will increase, allowing the solvent molecules to move rapidly and weaken/break the intermolecular forces that held the solute molecules together. The breakdown of the intermolecular forces brings about solubility.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

b.

the accuracy of the data.