A sample of helium gas containing (6.02 times 10^{2.3}) atoms at atmospheric pressure (left(1.01 times 10^{5} mathrm{~Pa}
Question:
A sample of helium gas containing \(6.02 \times 10^{2.3}\) atoms at atmospheric pressure \(\left(1.01 \times 10^{5} \mathrm{~Pa}\right)\) occupies a volume of \(22.4 \times 10^{-3} \mathrm{~m}^{3}\). The mass of a helium atom is \(6.646 \times 10^{-27} \mathrm{~kg}\). What is the rms speed of the helium atoms?
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We can find the rms speed of the helium atoms using the ideal gas law and the concept of root mean s...View the full answer
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