C4H10 has one more carbon than C3H8, therefore more surface area for London force to act on (intermolecular force), therefore higher boiling point, which means that it is easier to become liquified,
But wouldn't there be more energy required to overcome these IMF forces than necessary for C3H8?
Notice the data they gave you is for boiling points (so to get from liquid to gas). Using the table, it would be easier to liquidify C4H10 as opposed to C3H8 because its easier to achieve -1°C as opposed to -42°C
I'm doing IB - I don't think I'll be getting mocks at all before or after Christmas! But I'm going to by crying doing Maths everyday over Christmas; it's damn tough and I need to do it
Well I have gone from art college to general college, back to art college and now going back somewhere else for 6 months and start again in September. Been a crazy time but at least I have a sense of where I am going now.
I'm just wondering, how many of you are certain about which course you want to do? And how many of you have seriously thought about which universities you're going to go to? I haven't a clue where I'm going to apply for.