2. Consider all parts of the experiments that you have just performed. • What conclusions can you make about the relationship between the volume of a gas and its temperature?
• What conclusions can you make about the relationship between the volume of a gas and its pressure?
• What possible variables have you not accounted for? As you did the procedures, is it possible that the atmospheric pressure may have changed? If it did change over the course of your experiment, then how would your results have been affected?

The relationship between volume of a gas and temperature is given in Charles' law. It states that at constant pressure the volume of a gas is directly proportional to the temperature for a fixed amount of gas.

V/T = k

where V- volume , T - temperature and k - constant  

When temperature increases, the kinetic energy of molecules too increase and the gas molecules move faster and spread out more, hence they occupy more space which means volume increases when there's an increase in temperature

Explanation:

it is v / t equals k

Explanation:

if this helps you cannot get brainlist

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.