An ideal gas at 18.0 °C and a pressure of 2.83 x 105 Pa occupies a volume of 2.63 m3. (a) How many moles of gas are present? (b) If the volume is raised to 5.09 m3 and the temperature raised to 31.6 °C, what will be the pressure of the gas?
If N is the number of molecules then:
PV = NkT ---->
N = PV/(k T)
P = of 2.83 x 10^5 Pa
T = 291.15 K
V = 2.63 m^3
k = 1.38065*10^(-23)J K^(-1)
Calculate N and divide by 1 mole.
1 mole times the mass of one atomic mass unit is 1 gram.
1 atomic mass unit is 1.66054*10^(-27) kg ---->
1 mole is 6.02214*10^(23)
Remember: a mole is just a number just like a billion is a number!
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