Well you're missing out enthalpy of atomisation, mean bond enthalpies, enthalpy of hydration, enthalpy of solution, lattice enthalpy But yeah what you done so far is good
Here are my notes on Hess' Law and Hess Cycles, hope they help, if you can't read any parts let me know and I can type them up.
Edit: Would appreciate some feedback on the notes, just to see if they're missing out on anything. I do international as chem so I sat my unit 1 in January (and wrote that before the exam) and I'm not sure if I've missed out anything there.
Thankyou, it hasd made certain elements a lot clearer
guys....I genuinely do not understand Hess's Law cycles AT ALL.
I've tried and tried....
How did you guys manage to wrap your heads around it?
I've never really understood the point of drawing those diagrams, I find it easier to just reverse one of the equations to get the products on the right side etc. But you need to remember to flip the sign of the ΔH
guys....I genuinely do not understand Hess's Law cycles AT ALL.
I've tried and tried....
How did you guys manage to wrap your heads around it?
Don't worry, at AS level as long as you remember the specific equations for whether you have formation or combustion data you will be fine, I remember my teacher saying you could rely on them alone. Although at A2 you will have to have an understanding about it, however it should make more sense at that point in A2.
Out of the three following Intermolecular forces, whats the order of strength? -Electronegativity (permanent polar dipole-dipole) -Van der Waals', -Hydrogen Bonds
Out of the three following Intermolecular forces, whats the order of strength? -Electronegativity (permanent polar dipole-dipole) -Van der Waals', -Hydrogen Bonds
I would appreciate it if someone could explain to me why some salts are soluble in water while others such as lithium fluoride are not?
Thanks
the enthalpy of solution is positive and too endothermic, this means that there is a the entropy of the surroundings is negative, so despite the entropy of the stystem being postive, the total entropy of the system will be negative. Basically, for AS, the ionic bonds are too strong lol
Hey please can someone help on this question.. I just don't understand or enthalpy changes of combustion in general or of anything. Like when you do energy released and then switch over and do the opposite sign for temp released.. well all that makes no sense to me. Pls help!
Quesiton 2C. Can someone explain this to me. If the delta h is positive does that mean the reaction is endothermic. How do you know the reaction is to the right is my question basically.
If it was negative how would you know which way was exothermic or endothermic.
Is the way you do it by looking at the sign and saying the reaction to the right if negative = endothermic. If delta h is positive reaction to right = endothermic?
Also just tried doing it and got for bi) +56430 but I'm unsure whether it should be negative or not. For bii) 0.02 and for biii) 2820000 but that number seems so big so seems wrong Posted from TSR Mobile
Hey please can someone help on this question.. I just don't understand or enthalpy changes of combustion in general or of anything. Like when you do energy released and then switch over and do the opposite sign for temp released.. well all that makes no sense to me. Pls help!
Also just tried doing it and got for bi) +56430 but I'm unsure whether it should be negative or not. For bii) 0.02 and for biii) 2820000 but that number seems so big so seems wrong Posted from TSR Mobile
Divide by thousand to get kJ/mol First question is positive. Third question is negative