d. 4H30* (ag) + 2C1¯ (ag) + MnO2 (s) – Mn²+ (aq) + 6H2O(1) + Cl2 (g) [Mn²+ [Cl2] O Ke || 4 Mn²+ [H2O]°[Cl2] O Kc 4 H,O+CI-j° [MnO2] Mn?+ H2O][Cl2] O Ke H;O* [CIJ° [MnO2]

Complete and balance the following redox reaction in basic solution CIO3 (aq) + C204² (aq) → CIO2(g) + CO2(g) 14- 3- |2- O2+ 3+ 4+ 1 6. 7 8 9 0. O3 Os O, Do 12 14 7 9. (s) (1) (g) (aq) OH H2O ei H3O 4+ 2. +

Identify the type of each reaction in the copper cycle. Cu(NO3)2 (aq) + 2NaOH(aq) →→→ Cu(OH)2 (s) + 2 NaNO3 (aq) Choose... Cu (s) + 4HNO3(aq) →→ Cu(NO3)2 (aq) + 2 NO₂ (aq) + 2 H₂O (1) Choose... CuSO4 (aq) + Zn (s) → ZnSO4 (aq) + Cu(s) Choose... A Cu(OH)2 (s) → CuO (s) + H₂O (g) Choose... CuO (s) + H₂SO4 (aq) - → CuSO4 (aq) + H₂O (1) Choose... ▾

Complete the changes in concentrations for each of the following reactions. please tell or show how to solve the problems.     (b) Cu2SO4(s)    2 Cu+(aq) + SO42−(aq) Reaction Cu2SO4(s)   2 Cu+(aq) + SO42−(aq) relative change             +x (c) Cr(CN)3(s)    Cr3+(aq) + 3 CN−(aq) Reaction Cr(CN)3(s)   Cr3+(aq) + 3 CN−(aq) relative change     +x         (d) Fe(CN)Br(s)    Fe2+(aq) + CN−(aq) + Br−(aq) Reaction Fe(CN)Br(s)   Fe2+(aq) + CN−(aq) + Br−(aq) relative change             +x

why transition elements are able to form interestitial compounds ?

R = 8.314 mol·K F = 96,485 mot AG = AG° + RT · In(Q) ΔΕΔΕ-).In(O) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (1) 1.229 2 z" (aq) Z2 (s) + 2 e 3+ (aq) + 3 е 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e - 1.893 → M (s) A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate AG° in kJ/mol for this galvanic cell. Report your answer with 4 significant figures. You do not need to report units with your answer. If your value is negative, make sure to include a "-" symbol.

R = 8.314 mol·K F = 96,485 mol AG° + RT · In(Q) AE° () · In(Q) AG ΔΕ %3D Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e → 2 H20 (I0) 1.229 Z2 (s) + 2 e - → 2Z (aq) 0.426 (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M2+ (aq) + 2 e Н2 (в) + 2 ОН" (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 M MZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 10 Oxidation will occur at the while reduction will occur at the Possible answers are "anode" and "cathode".

Mn04 (aq) + SH"(aq) + 5e → Mn2"(aq) + 4H201) Cry0,2 (ag) + 6e → 2Cr*(aq) + 7H2O0) Cu2" +1.51 V +1.33 V *(aq)+2e Cu(s) (aq) + 2e Pb(s) (aq) + 2e→ Fe(s) +0.34 V -0.13 V Fe2+ Al3*(aq) + 3e → AI(3) -0.44 V -1.66 V Refer to Exhibit 17-1. Determine E cell for the electrochemical cell designated by the cell notation below. Al(3) | Al3* (ag) || Cu2*(aq) | Cu(s) O a. +12.0 V O b.+5.66 V Oc.-2.00 V O d.-1.32 V O e. +2.00 V

help  please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

Determine the covalency of the following and put them in decreasing order:  Br₂, SO₂, NH3, HCL