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Molar Mass Of A Gas
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Molar Mass of a Gas
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The density of gas with 336 g/mol at standard temperature and pressure would need to be D=m/volume so using pV=Nrt and solving the plugging back into the density equation you have a density of 2.4.
Atmospheric nitrogen is diatomic (N 2 ). The molar mass is 2x the molar mass of monatomic N. 2 x 14.01 = 28.02 g/mol = molar mass N 2 .
You are going to need to use the formula PV=nRT Then you are going to want to reformat it so that you solve for n (moles) n= PV/RT In this format you are going to want to use the R constant .08206 Plug in the numbers into the appropriate sp...
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final answer is 44.3g/mol Use the equation M= (mass/PV)(RT) and convert the given measurements into SI units e.g. 245mL into .245L and 29C into 302K
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The molar mass of hydrogen gas (H 2 ) is 2.0158g. Hydrogen gas is diatomic therefore it's formula is H 2 . The atomic mass of hydrogen is 1.0079g and multiplying by the two hydrogen atoms is equal to 2.0158g.
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The Molar Mass is 71.0 g
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Whenever you are referring to molar mass, the correct unit is in expressed in terms of grams. Since there are two atoms per molecule of chlorine, this would yield 2 Cl atoms per Cl molecule x 35.5 amu per Cl atom = 71.0 amu. This the molecu...
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rate of effusion of pure methan (CH4) gas is 47.8mL/min.
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I believe it would be Bromine. Bromine is a diatomic gas with a molar mass of 79.904g/mol. Since it's diatomic, it'll travel in pairs - so you double it's molecular mass.
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Don't know where you got that from because it makes no sense at all for many different reasons. 22.4 L is the molar volume of a gas at STP because 1 mole of any gas has a volume of 22.4 L at STP. It's definitely not the molar mass though.
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