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Extra Credit: Real vs Ideal Gases The van der Waals equation provides corrections to the ideal gas equation under conditions when assumptions from kinetic molecular theory are no longer valid. These corrections when applied to the ideal gas equation give the Van der Waals equation for real gas behaviour. (P + an²/V²)(V – nb) = nRT The constants a and b account for the effects of attraction that are present and the molecule, and are specific to each gas. Carbon dioxide gas (1.00 mole) at 373 K occupies 536 mL at 50.0 atmosphere pressure. (a) What is the calculated value of the pressure using (i) Ideal gas equation (ii) Van der Waals equation [Van der Waals constants for carbon dioxide: a = 3.61 L² atm mol?²; b = 0.0428 L mol?¹] (b) Is the pressure of the real gas higher or lower than that of the ideal gas? By what factor?

          Extra Credit: Real vs Ideal Gases

The van der Waals equation provides corrections to the ideal gas equation under conditions when assumptions from kinetic molecular theory are no longer valid. These corrections when applied to the ideal gas equation give the Van der Waals equation for real gas behaviour.

(P + an²/V²)(V – nb) = nRT

The constants a and b account for the effects of attraction that are present and the molecule, and are specific to each gas.

Carbon dioxide gas (1.00 mole) at 373 K occupies 536 mL at 50.0 atmosphere pressure.

(a) What is the calculated value of the pressure using

(i) Ideal gas equation
(ii) Van der Waals equation

[Van der Waals constants for carbon dioxide: a = 3.61 L² atm mol?²; b = 0.0428 L mol?¹]

(b) Is the pressure of the real gas higher or lower than that of the ideal gas? By what factor?

Extra Credit: Real vs Ideal Gases

The van der Waals equation provides corrections to the ideal gas equation under conditions when assumptions from kinetic molecular theory are no longer valid. These corrections when applied to the ideal gas equation give the Van der Waals equation for real gas behaviour.

(P + an²/V²)(V – nb) = nRT

The constants a and b account for the effects of attraction that are present and the molecule, and are specific to each gas.

Carbon dioxide gas (1.00 mole) at 373 K occupies 536 mL at 50.0 atmosphere pressure.

(a) What is the calculated value of the pressure using

(i) Ideal gas equation
(ii) Van der Waals equation

[Van der Waals constants for carbon dioxide: a = 3.61 L² atm mol?²; b = 0.0428 L mol?¹]

(b) Is the pressure of the real gas higher or lower than that of the ideal gas? By what factor?

Added by Ryan T.

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