For a volume of 100cc of nitrogen gas (N2) at a temperature of100°C and 1.0 ATM

Question

For a volume of 100cc of nitrogen gas (N2) at a temperature of100°C and 1.0 ATM pressure, find
(a) the number of moles, (b) the number of molecules, (c) the massin kg, (d) the density in kg/m3

If nitrogen is replaced by oxygen in the previous problem, which ofthe four items you calculated would
be different? Calculate them.

Explanation / Answer

we have : PV = nRT => the number of moles :   n = PV/RT =1.013x10^5*100x10^-6/(8.31*373) =3.27x10^-3mol the number of molecules : N = n*Na = 1.967x10^21 molecules the mass : M = m(N2)*N = 28*1.67x10^-27*1.967x10^21 =9.2x10^-5 kg the density : = M/V = 9.2x10^-5/100x10^-6 =0.92 kg/m3 For O2 : the number of mole is the same : n = 3.27x10^-3mol the number of molecules is the same also : N = 1.967x10^21 molecules the mass : M = N*m(O2) = 1.967x10^21*32*1.67x10^-27= 1.05x10^-4 kg the density : = M/V = 1.05kg/m3

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