A tank contains 0.831 mol of molecular nitrogen (N 2 ). Determine the mass (in g

Question

A tank contains 0.831 mol of molecular nitrogen (N2). Determine the mass (in grams) of nitrogen that must be removed from the tank in order to lower the pressure from 41.7 to 19.9 atm. Assume that the volume and temperature of the nitrogen in the tank do not change.

When solving PV=nRT and it is set up please explain all values used for V/RT=n/p

Solve out please

Explanation / Answer

PV = nRT => P/n = RT/V = constant P1/n1 = P2/n2 => 41.7/0.831 = 19.9/n2 => n2 = 0.3966 mole moles removed = 0.831 - 0.3966 = 0.4344 mole mass removed = 0.4344*(2*14) = 12.1632 g

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