Chapter 9: Q6 E (page 506)
A typical barometric pressure in Kansas City is 740 torr. What is this pressure in atmospheres, in millimeters of mercury, and in kilopascals?
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If the temperature of a fixed amount of a gas is doubled at constant volume, what happens to the pressure?
Question: Starting with the definition of rate of effusion and Graham’s finding relating rate and molar mass, show how to derive the Graham’s law equation, relating the relative rates of effusion for two gases to their molecular masses.
Question: When two cotton plugs, one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white ring of \({\rm{N}}{{\rm{H}}_{\rm{4}}}{\rm{Cl}}\) forms where gaseous \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) and gaseous \({\rm{HCl}}\) first come into contact. (Hint: Calculate the rates of diffusion for both \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) and \({\rm{HCl}}\), and find out how much faster \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) diffuses than \({\rm{HCl}}\).) \({\rm{N}}{{\rm{H}}_{\rm{3}}}{\rm{(g) + HCl(g)}} \to {\rm{N}}{{\rm{H}}_{\rm{4}}}{\rm{Cl(s)}}\)
At approximately what distance from the ammonia moistened plug does this occur?
Question: Heavy water, \({{\rm{D}}_{\rm{2}}}{\rm{O}}\) (molar mass\({\rm{ = 20}}{\rm{.03 gmo}}{{\rm{l}}^{{\rm{ - 1}}}}\)), can be separated from ordinary water, \({{\rm{H}}_{\rm{2}}}{\rm{O}}\) (molar mass\({\rm{ = 18}}{\rm{.01}}\)), as a result of the difference in the relative rates of diffusion of the molecules in the gas phase. Calculate the relative rates of diffusion of \({{\rm{H}}_{\rm{2}}}{\rm{O}}\) and \({{\rm{D}}_{\rm{2}}}{\rm{O}}\).
Iodine, I2, is a solid at room temperature but sublimes (converts from a solid into a gas) when warmed. What is the temperature in a 73.3mL bulb that contains 0.292 g of I2,vapour at a pressure of 0.462 atm?
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