Absolute zero and the ideal gas lawdata1. run pressure (kpa) temperature(°c)cold water 102.303 4.19room temperature of water 110.665 21.57warm water 116.111 34.35hot water 139.218 81.972. run pressure (kpa) temperature (°c)hot water 103.038 85.35cold water 76.65 8.05room temperature of water 83.549 26.44warm water 86.206 33.793. run pressure (kpa) temperature (°c)warm water 102.32 26.94hot water 104.862 32.97cold water 124.606 79.62room temperature of water 93.664 6.59diameter of sphere: 10.0cmq1.use your values to determine the number of moles n of air in the sphere. pay attention to the units! which run had the greatest number of moles of gas in the sphere? q2.give the numerical value of absolute zero that you measured including the uncertainty, the accepted value, and the percent difference between them. was the value you found lower or higher than accepted value? does the accepted value fall within the uncertainty of your measurement? why or why not? q3.do you think it is valid to assume that our linear continues to zero? or, more to the point, what would happen to our measurements if we continued cooling the volume (for example, by putting it in a bath of liquid nitrogen)? the gas is only "ideal" if the gas molecules do not interact with each other. luckily for us, this is the case with nitrogen and oxygen (the main components of air) at room temperature. however, if we were to cool the air way down, the molecules would move more slowly, allowing them to come closer together where they would interact with each other. (whether these interactions are attractive or repulsive depends on the molecules in question.) assuming that the air molecules would attract each other at low temperature, they would then tend to pull each other away from the walls of the container more than an ideal gas. do you think this would result in a higher or lower pressure vs that predicted by the ideal gas law?