An unknown gas shows a density of 2.4 gram per liter at 273^0 C and 1140 mm Hg pressure. What is the gram molecular mass of this gas?
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shedrick333
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There is a calculator at http://easycalculation.com/chemistry/molar-mass-ofgas.php that may help you.
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mwmovr40
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From the Ideal Gas Law we get
PV = nRT, where P is pressure, V is volume, n is number of moels, R is the Ideal Gas Constant, and T is the temperature in Kelvin.
Solving for n, we get the number of moles of gas (remembering to convert the pressure to ATM, and temperature to Kelvins).
n = PV/RT
n = 1.5ATM*1L/(0.0821 LATM/molK)(546K)
n = 0.033 moles.
molar mass = mass/moles = 2.4g/0.033mole = 72.7 g/mole