I have proofs and solution guidelines for every problem but no answers An ideal
ID: 1582687 • Letter: I
Question
I have proofs and solution guidelines for every problem but no answers An ideal gas at 17.0 C and a pressure of 1.54 105 Pa occupies a volume of 4.00 m3 (a) How many moles of gas are present? (b) If the volume is raised to 5.40 m3 and the temperature raised to 37.5° C, what will be the pressure of the gas? Pa At the start of a trip, a driver adjusts the absolute pressure in her tires to be 2.81 105 Pa when the outdoor temperature is 287 K. At the end of the trip she measures the pressure to be 3.00 105 Pa. Ignoring the expansion of the tires, find the air temperature inside the tires at the end of the trip. In a diesel engine, the piston compresses air at 302 K to a volume that is 0.0628 of the original volume and a pressure that is 48.7 times the original pressure. What is the temperature of the air after the compression? Oxygen for hospital patients is kept in special tanks, where the oxygen has a pressure of 63.0 atmospheres and a temperature of 295 K. The tanks are stored in a separate room, and the oxygen is pumped to the patient's room, where it is administered at a pressure of 1.00 atmosphere and a temperature of 297 K. What volume does 1.00 m3 of oxygen in the tanks occupy at the conditions in the patient's room? m3 A gas has a volume of 810.6 mL at-39.5 °C and 354.9 torr. What would be the new volume if the temperature is increased to 20.7 °C and the pressure increased to 582.2 torr? A clown at a birthday party has brought along a helium cylinder, with which he intends to fill balloons. When full, each balloon contains 0.034 m3 of helium at an absolute pressure of 1.2 105 Pa. The cylinder contains helium at an absolute pressure of 1.30-107 Pa and has a volume of 0.0031 m3 The temperature of the helium in the tank and in the balloons is the same and remains constant. What is the maximum number of balloons that can be filled? balloonsExplanation / Answer
1. P = 1.54 x 10^5 Pa
T = 273 + 17 = 290 K
V = 4 m^2
Applying ideal gas equation,
P V = n R T { R = 8.314}
n = P V / R T = 255.5 moles ....Ans
(B) P V / T = constant
(1.54 x 10^5) (4) / (290) = P (5.40)/(273 + 37.5)
P = 1.22 x 10^5 Pa .....Ans