I'd be an outlet so that i'd never run out of energy and power like batteries and generators do cx
The answer is 268.1 u....
<span>Answer:
A 1.00 L solution containing 3.00x10^-4 M Cu(NO3)2 and 2.40x10^-3 M ethylenediamine (en).
contains
0.000300 moles of Cu(NO3)2 and 0.00240 moles of ethylenediamine
by the formula Cu(en)2^2+
0.000300 moles of Cu(NO3)2 reacts with twice as many moles of en = 0.000600 mol of en
so, 0.00240 moles of ethylenediamine - 0.000600 mol of en reacted = 0.00180 mol en remains
by the formula Cu(en)2^2+
0.000300 moles of Cu(NO3)2 reacts to form an equal 0.000300 moles of Cu(en)2^2+
Kf for Cu(en)2^2+ is 1x10^20.
so
1 Cu+2 & 2 en --> Cu(en)2^2+
Kf = [Cu(en)2^2+] / [Cu+2] [en]^2
1x10^20. = [0.000300] / [Cu+2] [0.00180 ]^2
[Cu+2] = [0.000300] / (1x10^20) (3.24 e-6)
Cu+2 = 9.26 e-19 Molar
since your Kf has only 1 sig fig, you might be expected to round that off to 9 X 10^-19 Molar Cu+2</span>
Answer:
<u>The deviations are :</u>
- <u>The activation energy which changes with temperature</u>
- <u>The arrhenius constant which depends on the temperature</u>
Explanation:
- There are deviations from the Arrhenius law during the glass transition in all classes of glass-forming matter.
- The Arrhenius law predicts that the motion of the structural units (atoms, molecules, ions, etc.) should slow down at a slower rate through the glass transition than is experimentally observed.
- In other words, the structural units slow down at a faster rate than is predicted by the Arrhenius law.
- <em>This observation is made reasonable assuming that the units must overcome an energy barrier by means of a thermal activation energy. </em>
- The thermal energy must be high enough to allow for translational motion of the units <em>which leads to viscous flow of the material.</em>
- Both the Arrhenius activation energy and the rate constant k are experimentally determined, and represent macroscopic reaction-specific parameters <em>that are not simply related to threshold energies and the success of individual collisions at the molecular level. </em>
- Consider a particular collision (an elementary reaction) between molecules A and B. The collision angle, the relative translational energy, the internal (particularly vibrational) energy will all determine the chance that the collision will produce a product molecule AB.
- Macroscopic measurements of E(activation energy) and k(rate constant ) <em>are the result of many individual collisions with differing collision parameters. </em><em>They are averaged out to a macroscopic quantity.</em>
