New PDF release: Applied Physical Chemistry

By C. Heald, A. C. K. Smith (auth.)

ISBN-10: 1349016446

ISBN-13: 9781349016440

ISBN-10: 1349016462

ISBN-13: 9781349016464

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9 This example illustrates the procedure that can be used when it is desired to calculate the temperature of a gas. 0 m3 capacity is to be filled with 4000 mol of diethy1 ether and it is required to estimate the temperature above which the vessel must not be heated if a pressure of 20 MN m- 2 is not to be exceeded. 60 MN m -z and 467 K respectively. It is readily shown from the definition of z that the compressibility of ether at the maximum allowed pressure is 602/T. 28. 8; this yields a value of 4 7 8 for the product Tz, which is appreciably lower than the required value of 602.

1. 12 is more difficult since the equation is cubic; graphical solutions are usually suitable in calculations of this type. 50 MN m- 2 and at a temperature of 298 K. 38 x I0- 5 m3 mol- 1 respectively. 1 and this indicates the range of V values over which the graph should be plotted. 0802 m3 ; this last quantity is the volume required. 3 Other equations of state More accurate calculations require correspondingly more accurate, and necessarily more cumbersome, equations of state. 14) {3, 'Y and o can be calculated from published constants for the gas and the temperature.

5 kJ. 50 m 3 s- 1 results in a nitric oxide output of the same amount. 0 mol s- 1 . 38 MJ s- 1 . 8 mol of nitrogen enter the heat exchanger each second. 2 J K- 1 mol- 1 are the constant-pressure molar heat capacities of oxygen, nitrogen and ammonia respectively. 4 MJ for one second of flow. 0 MJ s- 1 must be supplied from an outside source of heat. One obvious application for thermochemistry is in the examination of combustion reactions relevant to fuels usage. 1 are the data used in these fuels examples.

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Applied Physical Chemistry by C. Heald, A. C. K. Smith (auth.)


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