posted by Ling on .
Consider the gold-platinum system which has a value of delta w of -4250 J/mole;
(a) Calculate the enthalpy of mixing for a solution of 10% platinum and 90% gold. Express your answer in units of kJ/mole.
(b) Is the dissolution of 10% platinum into gold an endothermic or an exothermic process?
i)Exothermic as the change in enthalpy is negative.
ii)Endothermic as the change in enthalpy is positive.
iii)Impossible to tell without considering the entropy of the system.
pls someone a) ?????????
-2.295 for a)
Please discuss how you arrived at that -2.295 figure rather than directly give that answer. If all of you just wanted that f.uc.k.ing certificate without understanding the material, then what you will get is only certificate not the knowledge and experience...
Please mind your own answers--and business.
He has got a point, though he did it a bit too aggressively. What he wants to know is, what are the formulas for working out these two questions? After all, a similar question could pop up in the final exam! To tell you the truth, i kinda miss how it was at the beginning of the course, with people taking to the forums and asking for help with the formulas, and pointing out any mistakes in other people's posted formulas. people wrote the most beautiful things then. *Sigh* These days, it's just "The Answer is X" on sites like these.