G.3 A glass vessel contains 28 g nitrogen gas. Assuming ideal behavior, which of the processes listed below would double the pressure exerted on the walls of the vessel? a) Adding enough mercury to fill one-half the container. b) Raising the temperature of the container from 30. o C to 60. o C. c) Raising the temperature of the container from -73 o C to 127 o C. d) Adding 28 g nitrogen gas (inert gas). Processes a, c, and d will all result in a doubling of the pressure. Process a has the effect of halving the volume, which would double the pressure (Boyle’s law). Process c doubles the pressure because the absolute temperature is doubled (from 200. K to 400. K). Process d doubles the pressure because the moles of gas are doubled (28 g N 2 is 1 mol of N 2 ). Process b won’t double the pressure since the absolute temperature is not doubled (303 K to 333 K). G.4 An ideal gas at 7 o C is in a spherical flexible container having a radius of 1.00 cm. The gas is heated at constant pressure to 88 o C. Determine the radius of the spherical container after the gas is heated. Because the container is flexible, P is assumed constant. The moles of gas present are also constant.
Gas Law Problems Key G.5 Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H 2 O 2 (aq) 2H 2 O(l) + O 2 (g) What volume of pure O 2 (g) collected at 27 o C and 746 Torr, would be generated by decomposition of 125 g of 50.0% by mass hydrogen peroxide solution? Ignore any water vapor that may be present.
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- Fall '08
- Chemistry, Gas Law Problems