1) The relationship between volume of a gas and its temperature, in Kelvin, assuming pressure is held constant is best shown by the statement; "The relationship is directly proportional, as temperature increases, volume increases in the same way."
2) The statement " an increase in pressure causes particles move closer together, decreasing the volume." explains the changes that occur when pressure is increased at constant temperature.
3) From the ideal gas law, the pressure increases as temperature increases
4) Following from Boyle's law; the volume decreases as the pressure increases.
5) The number of moles of each gas of each gas can be different.
Charles law states that; the volume of a given mass of gas is directly proportional to its temperature at constant pressure. This implies that, given a mass of gas, the temperature increases as the volume increases at constant temperature.
According to Boyle's law the volume of a given mass of gas is inversely proportional to its volume at constant temperature. This simply implies that as pressure increases as volume decreases(inverse proportionality and vice versa).
The pressure and temperature are directly proportional to each other when other variables are held constant.
From Avogadro's law, the volume of a given mass of gas is directly proportional to the number of moles( V α. n). Therefore, the number of moles of each gas of each gas can be different when the gases are held at the same pressure, volume, and temperature.
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