A storage tank contains 18.5 kg of nitrogen (N_2) at an absolute pressure of 3.00 atm. What will the pressure be if the nitrogen is replaced by an equal mass of CO_2?
From ideal gas equation,
PV = nRT
(P/n) = RT/V
No. of moles of N2 = 18.5 x 1000/28 = 660.71 moles
No. of moles of CO2 = 18.5 x 1000/44 = 420.45 moles
(3/660.71) = P'/420.45
P' = 1.91 atm
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A storage tank contains 18.5 kg of nitrogen (N_2) at an absolute pressure of 3.00 atm....
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