A storage tank at STP contains 26.3 kg of nitrogen (N2).
What is the pressure if an additional 27.7 kg of nitrogen is added without changing the temperature?
Using Ideal gas law:
PV = nRT
Step 1: find the volume of tank
V = nRT/P
n = number of moles of N2 = m/Mw = 26.3 kg/(28*10^-3 kg/mol) = 939.28 moles
R = 8.314
T = 0 C = 273 K
P = 1 atm = 1.01325*10^5 Pa, So
V = 939.28*8.314*273/(1.01325*10^5) = 21.04 m^3
Since temperature is constant, So
Now when 27.7 kg Nitrogen is added, then new number of moles will be:
n1 = m1/Mw = (26.3 + 27.7)/(28*10^-3) = 1928.57 moles
V1 = V, and T1 = T, So
P1 = n1*R*T1/V1
P1 = 1928.57*8.314*273/(21.04)
P1 = 208047.4 Pa = 2.08*10^5 Pa
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