Problem: Large amounts of nitrogen gas are used in the manufacture of ammonia, principally for use in fertilizers. Suppose 130.00 kg of N2(g) is stored in a 1400.0 L metal cylinder at 290 oC.Given that for N2, a = 1.39 L atm/mol2 and b = 0.0391 L/mol, calculate the pressure of the gas according to the van der Waals equation.

FREE Expert Solution

Step 1

n = 130.00 kg×103 g1 kg×1 mol28.02 g= 4640 mol


Step 2

P=nRTV-nb-an2V2


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Problem Details

Large amounts of nitrogen gas are used in the manufacture of ammonia, principally for use in fertilizers. Suppose 130.00 kg of N2(g) is stored in a 1400.0 L metal cylinder at 290 oC.

Given that for N2, a = 1.39 L atm/mol2 and b = 0.0391 L/mol, calculate the pressure of the gas according to the van der Waals equation.

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