1. A quantity of an ideal gas initially at atmospheric pressure is maintained at
ID: 1795234 • Letter: 1
Question
1. A quantity of an ideal gas initially at atmospheric pressure is maintained at a constant temperature while it is compressed to one-third of its volume. What is the final pressure of the gas? Pa 2. A Goodyear blimp typically contains 4700 m of helium (He) at an absolute pressure of 1.10 x 10 Pa. The temperature of the helium is 278 K. What is the mass (in kg) of the helium in the blimp?(The molar mass of Helium is 4.0026 g) kg 3. A rigid tank contains 54.5 g of chlorine gas (Cl2) at a temperature of 73 °C and an absolute pressure of 5.30 x 105 Pa. Later, the temperature of the tank has dropped to 34 °C and, due to a leak, the pressure has dropped to 3.90 x 105 Pa. How many grams of chlorine gas have leaked out of the tank? (The mass per mole of Cl, is 70.9 g/mol.) 4. Suppose a tank contains 610 m of neon (Ne) at an absolute pressure of 1.10 x 10° Pa. The temperature is changed from 293 K to 318 K. What is the increase in the internal energy of the neon? 5. Suppose there are two identical gas cylinders. One contains the monatomic gas neon (Ne), and the other contains an equal mass of the monatomic gas helium (He). The pressures in the cylinders are the same, but the temperatures are different. Determine the ratio KEN/ KEhe of the average kinetic energy of an atom of neon to the average kinetic energy of an atom of helium.Explanation / Answer
1) (1 atm) / (1/3) = 3.0 atm
2) pV = nRT
p = pressure
V = volume
n = number of moles
R = ideal Gas constant
T = absolute temperature
1.1 x 10^5 * 4700 = n * 8.314472 * 278
n = 223671.7
1 mole of helium is 4 grams, so 223671.7 moles would be 894686.8 grams or 894.6868 kg
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