A 9.439 mol sample of oxygen gas is maintained in a 0.8200 L container at 304.4 K. What is the pressure in atm calculated using the van der Waals' equation for O2 gas under these conditions

Explanation:

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In this case, since the Van der Waals' equation is used in order to analyze a gas slightly deviated from the ideal condition and is defined as:

Whereas a and b for oxygen are 0.0318 L/mol and 1.36 atm*L²/mol² respectively and represent the effective volume and the eventual interactions among the gas molecules. Moreover, the molar volume, vm, is:

Thus, the required pressure turns out:

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the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.