omework week-12: Intermolecular Forces \' g 3) The usual way to purify liquid hy

Question

omework week-12: Intermolecular Forces ' g 3) The usual way to purify liquid hydrocarbons is to distill them. That means heating e liquid from room temperature up to its boiling point, converting it to vapor, and then condensing the pure vapor. Suppose you want to distill heat capacity is 255.7 J/mol°C, and its heat of vaporization is 41 much heat input will be needed, assuming you start with octane at 100.0 g of octane. Its .0 KJ/mol. How 20°C? 4) Hydrogen bonds crea te the strongest intermolecular forces. Any hydrogen-oxygen (H-O) bond will form them. Consider the formula C2HeO, which could represent ethanol (bp 78°C) or dimethyl ether (bp -11°C). Explain why their boiling points are so different, even though they contain the same atoms. ethanol dimethyl ether H-C-C-O 5) When you add ice to your drink, the liquid water cools as the ice melts. The energy required to melt ice is 334 JIg, and you know that it takes 4.18 J to raise the temperature of one gram of water by 1°C. When one gram of water COOLS by 1°C, it transfers 4.18 J to something else, in this case, the ice. Assuming you add 25.0 g of ice to 200 mL of water at 20*C, what will the final temperature of your drink be?

Explanation / Answer

Ans 3 :

The boiling point of octane is 125oC

So the change in temperature will be ( 125 - 20) = 105oC

The molar mass of octane = 114.23 g/mol

So the number of mole = 100 / 114.23 = 0.875 moles

The heat energy to rise the temperature will be :

Q = n . C. Delta T

So putting all the values we get :

Q = 0.875 x 255.7 x 105

Q = 23492.4 J

Heat of vaporization = 0.875 x 41.0

= 35.875 KJ

So the total heat input = 23492.4 + 35875

= 59.367 KJ

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