Step 1

$\mathbf{n}\mathbf{}\mathbf{=}\mathbf{}\mathbf{130}\mathbf{.}\mathbf{00}\mathbf{}\mathbf{kg}\mathbf{\times}\frac{{\mathbf{10}}^{\mathbf{3}}\mathbf{}\mathbf{g}}{\mathbf{1}\mathbf{}\mathbf{kg}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}}{\mathbf{28}\mathbf{.}\mathbf{02}\mathbf{}\mathbf{g}}$= 4640 mol

Step 2

$\overline{){\mathbf{P}}{\mathbf{=}}\frac{\mathbf{n}\mathbf{R}\mathbf{T}}{\left(\mathbf{V}\mathbf{-}\mathbf{n}\mathbf{b}\right)}{\mathbf{-}}{\mathbf{a}}\frac{{\mathbf{n}}^{\mathbf{2}}}{{\mathbf{V}}^{\mathbf{2}}}}$

Large amounts of nitrogen gas are used in the manufacture of ammonia, principally for use in fertilizers. Suppose 130.00 kg of N_{2}(g) is stored in a 1400.0 L metal cylinder at 290 ^{o}C.

Given that for N_{2}, a = 1.39 L atm/mol^{2} and b = 0.0391 L/mol, calculate the pressure of the gas according to the van der Waals equation.

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