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Use the van der Waals equation to calculate the volume of 1.055 mol of neon at a pressure of 460.0 atm and a temperature of 375.0 K. (Use a = 0.211 L² .atm/mol? and b = 0.0171 L/mol for the van der Waals constants.) (Hint: One way to solve the van der Waals equation for V is to use successive approximations. Use the ideal gas law to get a preliminary estimate for V.) Express your answer in liters to three significant figures.V = ___ L

Respuesta :

The volume of 1.055 mol of neon at a pressure of 460.0 atm and a temperature of 375.0 K is 0.046 L

What is  the van der Waals equation?

The relationship between pressure, volume, temperature, and amount of actual gases is described by the Van der Waals equation. The equation for a real gas with 'n' moles is expressed as;

(P + an²/V²)(V - nb) = nRT

The formula can also be expressed as follows: Cube power of volume:

V = nRT/(P + an²/V²) -nb

Given that:  a = 0.211 L² .atm/mol,  b = 0.0171 L/mol, P = 460.0 atm T = 375.0 K, n = 1.055

Now from ideal gas equation V = nRT/P we get:

V = (1.055×0.082×375)/460.0 L

= 0.0705 L

Now from the van der Waals equation:

V =  (1.055×0.082×375)/(460.0 + 0.211×1.055²/0.0705²) - (1.055×0.0171)

= 0.046 L

Hence, volume of the gas is 0.046 L.

Learn more about the van der Waals equation here:

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