Triglycerides are broken down into smaller pieces (with the help of lipases) to be transported then reassembled where needed.
i see, so why are unsaturated fatty acids found in plant fats? anything to do with melting point at all?
also (very basic question ) why can haloalkane molecules, with a permanent dipole, create an induced dipole in triglycerides but water molecules can't?
Triglycerides are broken down into smaller pieces (with the help of lipases) to be transported then reassembled where needed.
edit: oh I see your point sorry, these monofatty acids too have a high melting point - I guess they must be in some sort of solution in the lymph system?
i've just looked up lymph system, i had no idea what it was but i take it the fatty acids are in an environment which allows them to be transported as liquids... if you figure out about the water solubility thing please let me know (unless it's too complicated), i'm sure i don't need to i'm just interested ( lol). thank you for help.
i've just looked up lymph system, i had no idea what it was but i take it the fatty acids are in an environment which allows them to be transported as liquids.
Pretty much yeah. If you look up "chyle" instead of lymph you'll find better information. It's basically lymph of the digestive system (though there is more to it) which is very rich in fatty acids and triglycerides.
it's just sometimes I get confused as to why for example NH3 would be times 3 but 2NH3 is times 6. Is there any rules for like determining how many times to multiply things by e.g. with H20 it's times by 2 and with 2H20 it's times by 4. I guess it's not that difficult to see why but I just get confused easily
Thanks for that though I was hoping you could help me with this:
use the following equation and the data from the table above(it's the data I gave in my first question) to calculate a value for the enthalpy of ethane:
C2H4 + H2 -----> C2H6
DeltaH = -136 kJmol^-1
It has the bonds of the equation drawn out btw and if you like I can draw them if you need to see
http://store.aqa.org.uk/qual/gceasa/qp-ms/AQA-CHM2-W-QP-JAN06.PDF According to question 1)(b) on that exam paper, the mean bond enthalpy for a C-H bond is 412. As all the other data in the question is identical to the data you've been given (C=C and C-C), I think it's safe to use that.
Ah yes I don't have the C-H it's told me I need to calculate it-find it out!
Seeing as they've given me the enthalpy change I think they want me to work out something I don't know (the C-H bond enthalpy in Ethane) from things I do know: the above data and the enthalpy change which is -136
But I have no idea how to !!! Because it doesn't want me to find the bonds formed it wants just one value in ethane - the C-H so does that mean I just divide by 6 once I've find out the bonds made in ethane?
If this doesn't make sense....I'm sorry and I'll repeat the question
Ah yes I don't have the C-H it's told me I need to calculate it-find it out!
Seeing as they've given me the enthalpy change I think they want me to work out something I don't know (the C-H bond enthalpy in Ethane) from things I do know: the above data and the enthalpy change which is -136
But I have no idea how to !!! Because it doesn't want me to find the bonds formed it wants just one value in ethane - the C-H so does that mean I just divide by 6 once I've find out the bonds made in ethane?
If this doesn't make sense....I'm sorry and I'll repeat the question
I'll post a (potentially helpful ) reply in a few minutes