Chapter 9: Q91E (page 512)
Question: Can the speed of a given molecule in a gas double at constant temperature? Explain your answer.
Yes, the speed of a given molecule in a gas doubles at constant temperature due to internal collisions.
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A sample of gas isolated from unrefined petroleum contains \({\rm{90}}{\rm{.0\% C}}{{\rm{H}}_{\rm{4}}}{\rm{, 8}}{\rm{.9\% }}{{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{6}}}{\rm{, and 1}}{\rm{.1\% }}{{\rm{C}}_{\rm{3}}}{{\rm{H}}_{\rm{8}}}\) at a total pressure of\({\rm{307}}{\rm{.2 kPa}}\). What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.)
Question: Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behaviour? Explain.
(a) high pressure, small volume
(b) high temperature, low pressure
(c) low temperature, high pressure
A typical barometric pressure in Kansas City is 740 torr. What is this pressure in atmospheres, in millimeters of mercury, and in kilopascals?
Question: A 0.245L flask contains 0.467 mol \({\rm{C}}{{\rm{O}}_{\rm{2}}}\) at 1590C. Calculate the pressure:
(a) using the ideal gas law
(b) using the van der Waals equation
(c) Explain the reason for the difference.
(d) Identify which correction (that for \({\rm{P}}\) or \({\rm{V}}\)) is dominant and why.
Question: During the discussion of gaseous diffusion for enriching uranium, it was claimed that \(^{{\rm{235}}}{{\rm{U}}_{\rm{6}}}\) diffuses 0.4% faster than\(^{{\rm{235}}}{{\rm{U}}_{\rm{6}}}\). Show the calculation that supports this value. The molar mass of \(^{{\rm{235}}}{{\rm{U}}_{\rm{6}}}{\rm{ = 235}}{\rm{.043930 + 6 \times 18}}{\rm{.998403 = 349}}{\rm{.034348 g/mol}}\), and the molar mass of \(^{{\rm{238}}}{{\rm{U}}_{\rm{6}}}{\rm{ = 238}}{\rm{.050788 + 6 \times 18}}{\rm{.998403 = 352}}{\rm{.041206 g/mol}}\).
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