Calculate the concentration of the chromic ion in the cell which has an electrode potential of 0.688 at 298.15 K for the given reaction: Cr2O7 2 –(aq) + 14 H+ (aq) + 6 I – 1 (aq) → 2 Cr 3+(aq) + 3I2(s) + 7 H2O(l)
When [Cr2O7 2 – ] = 2.25 M; [H+] = 1.0 M ; [I – 1 ] = 1.0 M ; [H2O] = 1.0 x 10 – 5 M

Calculate the Gibbs free-energy and the standard Gibbs Free-Energy occur in the system

Determine the  wavelength of light emitted when an electron  in an li2+ ion  makes a transition from an orbital with n  =  6 to an orbital with n  = 5.

Hairy thick gross thing? idk

Answerd. may include all of these are many definitions of bases: the  brønsted-lowry definition of acids and bases says that bases are proton acceptors.the arrhenius definition of acids and bases says that bases increase [oh⁻] in solution (thereby producing oh⁻ ions)the lewis definition of acids and bases says that bases donate electron pairs.therefore, the sensible answer is that a base may include all of the described characteristics.

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.