A 1.000 atm of dry Nitrogen gas (N2) is placed in a container with a pinhole opening on its side. The gas leaks from the container 2.283 times faster than the 1.000 atm of an unknown gas placed in the same apparatus. Which of these species could be the unknown gas?
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- The spherical gas tank is fabricated by bolting together two hemispherical thin shells of thickness 30 mm. The gas contained in the tank is under a gauge pressure of 2.5 MPa. If the tank has an inner diameter of 8 m and is sealed with 900 bolts each 20 mm in diameter, determine the internal force carried by each bolt.Oxygen with mass of m1=6 g and temperature T1=300 K is in a container under pressure p1= 9.66·105 Pa. If an unknown gas with mass m2= 3 g and temperature T2=330 K is placed in the same container, then the gas is under pressure p2=9·105 Pa. Find the molar mass of the unknown gas.Two glass containers, of equal volume each hold a mole of gas. Container 1 is filled with hydrogen gas (molar mass 2 g / mol), and Container 2 holds helium (molar mass 4 g / mol). If the pressure of the gas in Container 1 equals the pressure of the gas in Container 2, which of the following is true? (a) The temperature of the gas in Container 1 is lower than the temperature of the gas in Container 2. (b) The temperature of the gas in Container 1 is greater than the temperature of the gas in Container 2. (c) The value of R for the gas in Container 1 is ½ the value of R for the gas in Container 2. (d) The rms speed of the gas molecules in Container 1 is lower than the rms speed of the gas molecules in Container 2. (e) The rms speed of the gas molecules in Container 1 is greater than the rms speed of the gas molecules in Container 2.
- One mole of oxygen gas is at Three arterial geometries are shown in the figure, including a healthy blood vessel (i), a constricted blood vessel (ii), and a blood vessel with an aneurysm (a balloon-like bulge; (iii)). The speed of the blood at point ① in all three vessels is 40.0 cm/s.a pressure of 9.00 atm and a temperature of 38.0°C.Consider two containers with the same volume and temperature. The first container is labelled "Dry" and holds "dry" air = a ratio of nitrogen (N2) and oxygen (O2). The second container is labelled "Humid" and holds "moist" air = the SAME ratio of nitrogen and oxygen, but also contains water (H2O) vapor. According to the ideal gas law, if the pressures are equal, the weight of the gas inside the "Dry" container will beConsider the following experiment: 1.0 atm 1.0 mol N₂(g) 1.0 atm 3.0 mol H₂(g) ? The reaction chamber is initially divided by a partition into two unequal parts, as shown on the left side of the figure. The smaller volume contains 1.0 mol of N₂(g) at a pressure of 1.0 atm, while the larger volume contains 3.0 mol of H₂(g) at a pressure of 1.0 atm. The partition is removed, and the following reaction is carried out to completion in the combined volume shown on the right side of the figure: N₂(g) + 3 H₂(g) → 2 NH3(g). What quantities of which gases will be found in the reaction chamber after the completion of the reaction? (That is, what does the question mark on the right side of the figure stand for?) 0.5 mol N₂(g) 0.5 mol N₂(g) 0.0 mol N₂(g) 0.0 mol N₂(g) 0.0 mol N₂(g) 1.5 mol H₂(g) 1.5 mol H₂(g) 0.0 mol H₂(g) 0.0 mol H₂(g) 0.0 mol H₂(g) 2.0 mol NH3(g) 1.0 mol NH3(g) 2.0 mol NH3(g) 4.0 mol NH3(g) 1.0 mol NH3(g)