The van der Waals equation is a modification of the ideal gas equation. What two factors does this equation account for? A. (1) Real gas molecules exert forces on each other. (2) Gas molecules have energy. B. (1) Real gas molecules exert ionic forces on each other. (2) Gas molecules have energy C. (1) Real gas molecules exert forces on each other. (2) Gas molecules have volume. D. (1) Real gas molecules exert ionic forces on each other. (2) Gas molecules have volume. E. None of the above have BOTH of the two factors accurately stated HINT: Check Van der Waals equation.

The factor n^2a/V^2 accounts for the attractive forces between the gases molecules whereas nb accounts for the decrease in volume occupied by the gas. Therefore, correct option would be E. None of the above have BOTH of the two factors accurately stated

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pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-11-21T08:00:45+01:00

The correction of Van Der Waal to the ideal gas equation is that; real gas molecules exert forces on each other and that gas molecules have volume.

Van Der Waal (1873) proposed a modification to the ideal gas equation; PV = nRT. The ideal gas law assumes that molecules of gases do not have a definite volume but occupies the same volume as the container and do not exert any attractive forces on each other.

However, Van Der Waal introduced two major corrections to the ideal gas equation;

The gas molecules have real volume, V - nb gives the volume of the container that is inaccessible to the gas molecules.

The second correction has to do with the fact that the gases actually exert an attractive force on each other. The real pressure of the gas is less than the ideal pressure of the gas which is captured in the term; P + an^2/V^2.

Hence, the ideal gas equation is now written as;

[tex](P + \frac{an^2}{V^2}) (V - nb) = nRT[/tex]

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