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whar paticles in the compound contruibt to charge to form Cu2+ ion in Cu(H2o)62+
Cu(OH)2 (s)
CuO(s)
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- What is the enthalpy when 65.0 g of Cu2O is oxidized to CuO?2 Cu2O(s) + O2(g) --> 4 CuO dH = -288 kJ/molComplete the following reactions below. If no reaction occurred, write NR. Mg(s) + MgSO4(aq) -> Mg(s) + CusO4(aq) –> Cu(s) + MgSO4(aq) ->Given the enthalpy changes for the following reactions, calculate AH for CO C(gaphite) + 1/20 CO C(gaphite) + O → CO CO+ 1/202 → CO -> AH: = -393.5 kJ AH =-283.0 J
- Complete the following reactions below. If no reaction occurred, write NR. Cu(s) + CusO4(aq) –> Cu(s) + ZnSO4(aq) -> Zn(s) + ZnSO4(aq) - Zn(s) + CuSO4(aq) ->One of the steps for refining silver involves converting silver into dicyanoargenate(I) ions: 4Ag(s) + 8CN−(aq) + O2(g) + 2H2O(l) ⟶ 4[Ag(CN)2]−(aq) + 4OH−(aq)Explain why oxygen must be present to carry out the reaction. Why does the reaction not occur as: 4Ag(s) + 8CN−(aq) ⟶ 4[Ag(CN)2−(aq)?Cu20 + Cu,O |Cu +co CO2 Cu = Cu = C = C =
- Fe+Pb(NO3)2Calculate AH for the following reaction, FeO(s) + CO(g) -----> Fe(s) + CO2(g), from the following data, Fe2O3(s) + 3CO(g) -----> 2Fe(s) + 3CO2(g) 3Fe2O3(s) + CO(g) > 2FE3O4(s) + CO2(g) Fe;O4(s) + CO(g) AH = -23 KJ AH = -39 KJ --- -- -----> 3FeO(s) + CO2(g) AH =+18 KJ %3DCalculate ∆o for [Co(H2O)6]2+ in units of kJ.
- The following oxidation-reduction reactions take place in basic medium. For each reaction, (i) Assign oxidation state for each atom in the equation; (ii) Indicate oxidation half-equation and reduction half-equation; (iii) Balance the equation by half-equation method; (iv) Indicate which reactant is oxidizing agent and which reducing agent. (v) State and verify whether the pH of the medium decreases, increases, or remains constant as the reaction proceeds.c) Calculate the nominal masses of following ions and indicate whether they are odd-electron ions or even- electron ions: (i) CH;N+ (ii) H3O+ (iii)(f) Potassium permanganate (g) Sodium hypochlorite (h) Beryllium bicarbonate (1) Ammonium dichromate (G) Iron (II) chloride