Need Help? Read it 1.66 points SerCP 11 10 P062 My N Before beginning a long tri

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Need Help? Read it 1.66 points SerCP 11 10 P062 My N Before beginning a long trip on a hot day, a driver inflates an automobile t he end of the trip, the gauge pressure has increased to 2.08 atm re to a gauge pressure of 1.78 atm at 300 K. At (a) Assuming the volume has remained constant, what is the temperature of the air inside the tire? (b) What percentage of the original mass of air in the tire should be released so the pressure returns to its original value? Assume the temperature remains at the value found in part (a) and the volume of the tire remains constant as air is released. Need Help? L Read bmit Answer Save Progress My Note 1.66 points SerCP11 11 P010 A 1.75-g copper coin at 22.5°C drops 45.0 m to the ground Type here to search

Explanation / Answer

The pressure in the ideal gas law is the ABSOLUTE pressure, not the gauge pressure, so you have to add 1 atm to BOTH readings. The pressure ratio is then 3..08/2.78 = 1.1079

and the final temperature is 300 x 1.1079 = 332.4 K.

Second:
Nfin Tfin = Nin Tin => about 9.74 %

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