AP Chemistry Question of the Day --31

Welcome back to my blog. Here comes the answer to question 30 I posted yesterday. The correct answer is C. 

Water is a very polar molecule while hydrocarbons of high molecular weight are unpolar compounds. According to "Like dissolves like" Rule, The solubility of high molecular hydrocarbons will be very low in water.
Due to hydrogen bonding, water has a higher density as a liquid than as a solid, because the lattice structure in ice restricted the number of hydrogen bonding while in liquid water, the maximum hydrogen bonding could be achieved. Thus A and B are correct. Answer D is also correct because when we write the Lewis structure of water, the central oxygen atom has two bonds connected to hydrogen and two lone pairs of electrons. The central oxygen atom is sp3 hybridized and takes tetrahedron geometry. As the two lone pair electrons are not visible, the molecule appears as a bent shape.

Following is Question 31 of the series. 

31. Which of the following statements accounts for the observation that, at 300 K and 10 atm, the molar volume of C2H6(g) is less than that of H2(g)? 

A C2H6 molecules are smaller than H2 molecules. 
B The average kinetic energy of H2 molecules is greater than that of C2H6 molecules. 
C The average kinetic energy of H2 molecules is less than that of C2H6 molecules. 
D The intermolecular attractions in C2H6(g) are weaker than they are in H2(g). 
E The intermolecular attractions in C2H6(g) are stronger than they are in H2(g). 

I will post the answer and explanation tomorrow. 

Thank you very much for reading my post, I am available to discuss any topics in AP chemistry. Please give me a call at 604-808-6827 or email me at vancouverchemistrytutor@gmail.com. My website is located at www.vancouverchemistrytutor.com.

Regards!