Consider four 1L flasks labeled A, B, C, and D filled with the ideal gases He,...
Consider four 1L flasks labeled A, B, C, and D filled with the ideal gases He, Ne, Kr, and Xe, respectively, each at STP. Assuming ideal gas behavior, which of these four flasks contains the greatest quantity (in moles) of gas?
Homework Answers
At STP (Standard Temperature and Pressure), one mole of any ideal gas occupies 22.4 liters. Therefore, to determine which flask contains the greatest quantity of gas in moles, we need to calculate the number of moles of gas in each flask based on its volume.
Given: Flask A: He gas in 1L flask Flask B: Ne gas in 1L flask Flask C: Kr gas in 1L flask Flask D: Xe gas in 1L flask
Since all the flasks have the same volume of 1L, the flask with the gas that has the highest molar mass will contain the greatest quantity of gas in moles. This is because the molar mass is directly proportional to the number of moles of gas.
The molar masses of the gases are as follows: He: 4.0026 g/mol Ne: 20.1797 g/mol Kr: 83.798 g/mol Xe: 131.293 g/mol
Comparing the molar masses, we can see that Xe has the highest molar mass. Therefore, Flask D, which contains Xe gas, will have the greatest quantity of gas in moles.
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