For carbon dioxide gas the constants in the van der Waals equation are = 0.364 J
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For carbon dioxide gas the constants in the van der Waals equation are α = 0.364 J · m3/mol2 and
(a) If 1.00 mol of gas at 350 K is confined to a volume of find the pressure of the gas using the ideal-gas equation and the van der Waals equation.
(b) Which equation gives a lower pressure? Why? What is the percentage difference of the van der Waals equation result from the ideal-gas equation result?
(c) The gas is kept at the same temperature as it expands to a volume of Repeat the calculations of parts (a) and (b).
(d) Explain how your calculations show that the van der Waals equation is equivalent to the ideal-gas equation if is small.
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University Physics with Modern Physics
ISBN: 978-0321696861
13th edition
Authors: Hugh D. Young, Roger A. Freedman, A. Lewis Ford
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