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

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

Step 2

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

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