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Chapter 6: Problem 36
What is the molar mass of a gas found to have a density of \(0.841 \mathrm{g} / \mathrm{L}\) at \(415 \mathrm{K}\) and 725 Torr?
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A 10.0 g sample of a gas has a volume of \(5.25 \mathrm{L}\) at \(25^{\circ} \mathrm{C}\) and \(762 \mathrm{mm} \mathrm{Hg} .\) If \(2.5 \mathrm{g}\) of the same gas is added to this constant 5.25 L volume and the temperature raised to \(62^{\circ} \mathrm{C},\) what is the new gas pressure?
A 34.0 L cylinder contains \(305 \mathrm{g} \mathrm{O}_{2}(\mathrm{g})\) at \(22^{\circ} \mathrm{C} .\) How many grams of \(\mathrm{O}_{2}(\mathrm{g})\) must be released to reduce the pressure in the cylinder to 1.15 atm if the temperature remains constant?
A sample of \(\mathrm{O}_{2}(\mathrm{g})\) has a volume of \(26.7 \mathrm{L}\) at 762 Torr. What is the new volume if, with the temperature and amount of gas held constant, the pressure is (a) lowered to 385 Torr; (b) increased to 3.68 atm?
The equation \(d / P=M / R T,\) which can be derived from equation \((6.14),\) suggests that the ratio of the density \((d)\) to pressure (P) of a gas at constant temperature should be a constant. The gas density data at the end of this question were obtained for \(\mathrm{O}_{2}(\mathrm{g})\) at various pressures at \(273.15 \mathrm{K}\) (a) Calculate values of \(d / P,\) and with a graph or by other means determine the ideal value of the term \(d / P\) for \(\mathrm{O}_{2}(\mathrm{g})\) at \(273.15 \mathrm{K}\) [Hint: The ideal value is that associated with a perfect (ideal) gas.] (b) Use the value of \(d / P\) from part (a) to calculate a precise value for the atomic mass of oxygen, and compare this value with that listed on the inside front cover. $$\begin{array}{lllll} P, \mathrm{mmHg}: & 760.00 & 570.00 & 380.00 & 190.00 \\ d, \mathrm{g} / \mathrm{L}: & 1.428962 & 1.071485 & 0.714154 & 0.356985 \end{array}$$
Gas cylinder A has a volume of 48.2 L and contains \(\mathrm{N}_{2}(\mathrm{g})\) at 8.35 atm at \(25^{\circ} \mathrm{C} .\) Gas cylinder \(\mathrm{B},\) of unknown volume, contains \(\mathrm{He}(\mathrm{g})\) at 9.50 atm and \(25^{\circ} \mathrm{C} .\) When the two cylinders are connected and the gases mixed, the pressure in each cylinder becomes 8.71 atm. What is the volume of cylinder \(\mathrm{B} ?\)
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