t Ideal versus Real Gases The ideal gas law describes the relationship among the

Question

t Ideal versus Real Gases The ideal gas law describes the relationship among the volume of an ideal gas (V) its pressure (P. its absolute temperature (T), and number of moles n). Under standard PV nRT properties for conditions, the ideal gas law does a good job of approximating these any gas. However the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van der Waals equation corrects for these factors with the constants a and b which are unique to each substance: The gas constant R equal to 0.08206 L. atm/(K.mol). Idea In the how th Part E For Exp

Explanation / Answer

Solution:

The computation are expresssed below,

part A

P = 1.00 atm, T = 25 C = 298 K, V = 3.00L, R =0.0821 L-atm/mol-K

n = PV/RT = (1*3) / (0.0821*298) = 0.1227 moles

mass of NH3 = 17.031 g/mol * 0.1227 mol = 2.0897 gm

part B

n = 1.00 mol, V = 0.5 L, T = 29 C = 302 K, a = 1.345, b = 0.03219

(P+ (an2/V2))(V-nb) =nRT

by plugging values we get,

(P+(1.3445*12 /0.52))(0.5 - 1(0.03219)) = (1*0.0821*302)

P = 47.6226 atm

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