In Sample Exercise 10.16, we found that one mole of Cl2confined to 22.41 L at 0 °C deviated slightly from idealbehavior. Calculate the pressure exerted by 1.00 mol Cl2confined to a smaller volume, 5.00 L, at 25 °C. (a) First usethe ideal-gas equation and (b) then use the van der Waalsequation for your calculation. (Values for the van der Waalsconstants are given in Table 10.3.) (c) Why is the differencebetween the result for an ideal gas and that calculated usingthe van der Waals equation greater when the gas is confinedto 5.00 L compared to 22.4 L?
In Sample Exercise 10.16, we found that one mole of Cl2confined to 22.41 L at 0 °C deviated slightly from idealbehavior. Calculate the pressure exerted by 1.00 mol Cl2confined to a smaller volume, 5.00 L, at 25 °C. (a) First usethe ideal-gas equation and (b) then use the van der Waalsequation for your calculation. (Values for the van der Waalsconstants are given in Table 10.3.) (c) Why is the differencebetween the result for an ideal gas and that calculated usingthe van der Waals equation greater when the gas is confinedto 5.00 L compared to 22.4 L?
Chapter5: Gases
Section: Chapter Questions
Problem 152CP: You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted...
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Question
In Sample Exercise 10.16, we found that one mole of Cl2
confined to 22.41 L at 0 °C deviated slightly from ideal
behavior. Calculate the pressure exerted by 1.00 mol Cl2
confined to a smaller volume, 5.00 L, at 25 °C. (a) First use
the ideal-gas equation and (b) then use the van der Waals
equation for your calculation. (Values for the van der Waals
constants are given in Table 10.3.) (c) Why is the difference
between the result for an ideal gas and that calculated using
the van der Waals equation greater when the gas is confined
to 5.00 L compared to 22.4 L?
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