<p>collisions with the container are elastic. </p>
<p>Chromates are insoluble... not sure for permanganate, but I think it's insoluble.</p>
<p>...obviously, except for group 1a and ammonia (well that applies to everything)</p>
<p>what is a spontaneous reaction? anything that have a negative free energy? so is O2+H2=H20 a spontaneous reaction even though they don't react until activation energy is applied?</p>
<p>What are some ions that give color in solution? I know Cu=blue, Cr=green (?), iron=red/orange, permaganate=purple. What are some others?</p>
<p>I think K=green also (or am I thinking of flame test?)</p>
<p>youknowme, i've never seen the spontanaeity of that reaction, but it's totally possible for something to be thermodynamically spontaneous and not react. Are you sure it's spontaneous? That would have to be really exothermic in order to overcome the loss of entropy.</p>
<p>whats the deal with complex ions? what are the typical reactants in complex ion reactions? ex Ni and NH3?</p>
<p>transition metals with ammonia, OH-, CN-, or SCN- form complex ions. generally the number of ligands will be twice as much as the charge on the metal ion.</p>
<p>Cu^2+ +NH3 forms Cu(NH3)4^2+</p>
<p>for # 1, i dont think it is choice 3, because for slower reactions, the activation energy should be higher, thus requiring more energy to get going while faster has smaller activation energies because the reactions dont need as much energy and can break old bonds/make new bonds more rapidly (hence faster reaction)</p>
<p>er, for this one
"I have a couple of questions</p>
<ol>
<li>Activation energy for an elementary process</li>
</ol>
<p>1) Is part of the net enthalpy change for the reaction
2) None of these
3) Is smaller for slower reactions and larger for faster reactions
4) Is the energy required to produce the transition state from the reactants "</p>
<p>way back at reply #12</p>
<p>eeperkblah ~
I will say 4.
My question:
C2H7OH + ____ O2 --> __ CO2 + ___ H20</p>
<p>One mole of oxygen was reacted. What is the number of moles of 02 needed?</p>
<p>err, question. what was supersaturated, undersaturated (such thing? don't remember) and saturated?</p>
<p>Supersaturated - when a solution is filled to more than capacity (only possible for solids in liquids at high temps & low pressure)</p>
<p>saturated - when a solution is filled to capacity</p>
<p>undersaturated - when a solution is filled to less than capacity</p>
<p>What are ideal gas circumstances?</p>
<p>ideal gases are ideal at high temperatures and low pressures</p>
<p>ideal at high temps and low pressure</p>
<p>Does anyone know how common coordinate compound nomenclature will be? Our teacher touched on the subject for about 5 minutes so I'm not sure whether or not to be worried about it.</p>
<p>it might be part of equation writing and even then you have eight reactions to choose from, I'm sure if you don't know that one then there'll be another.</p>
<p>I wouldn't worry about it.</p>
<p>Is that the complex ion stuff? Can you give me an example...I may be able to explain it.</p>