posted by ACDub on .
When the oxide of generic metal M is heated at 25.0 °C, only a negligible amount of M is produced. MO2(s)<-->M(s)+O2(g) DeltaS= 287.5 kJ/mol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s). MO2(s)+C(s)<-->M(s)+CO2(g) What is the thermodynamic equilbrium constant for the coupled reaction?
Didn't I do this for you last week? As I remember you didn't understand my explanation. Or am I wrong?
It's the first time I ask this question on here actually.
Will you check that dS = -287.5? I may have it mixed up with another problem but I seem to remember that as being delta G or something like that but not dS. Thanks.
I looked at one of your description of one of the previous questions asked that are similar to mine and it made perfect sense. Thanks!