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7. Complete and balance the following equations: a) Ag CrOA(s) + HNO3(aq) b) AgCI(s) +NH3(aq)> c)...
7.40 Balance each of the following chemical equations: a. Zn(s) + HNO3(aq) H(g) + Zn(NO3)2(aq) b. Al(s) + H2SO4(aq) → H2(g) + Alz(SO2)3(aq) c. K SO,(aq) + BaCl(aq) → BaSO 9) + KCl(aq) d. CaCO3(s) — — Cao(s) + CO2(g) a. Zn(s) + HNO3(aq) —H2(g) + Zn(NO3)2(aq) b. Al(s) + H2SO4(aq) —> H2(g) + Al(SO4)3(aq) I
Account for your observations. Consider the following equilibria: Ag^+(aq)+Cl^-(aq)<->AgCl(s) Ag^+(aq)+2NH3(aq)<->[Ag(NH3)2]^+(aq) NH3(aq)+H^+(aq)<->NH4^+(aq) Observations: adding NaCl: went from clear to a white solution adding NH3: went from white solution to. clear solution adding HNO3: solution warmed up
Complete and balance the following equations I_2 (s) + OC^- (ag) rightarrow IO_3^- (aq) + Cl^- (aq) (acidic solution) Express your answer as a chemical equation. Identify all of the phases in your answer.
Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1 - 131.2 - 109.8 - 104.0 -96.9 (a) Calculate AG rn for the dissolution of AgCl(s). (b) Calculate the solubility-product constant of AgCl Number Number kJ mol (c) Calculate Δ3rxn for the dissolution of AgBr(s). (d) Calculate the solubility-product constant of AgBr Number Number kJ mol
1. Complete and balance the following equations: (a) C3H (g) + O2(E)-> (spark) (b) NazCr2O7.2H2O(s) ->(heat) (c) HF(aq) + Ca(OH)2(aq)->
Part 1 The Balanced Equilibrium Equations: Reactant(s) Product(s) Fe3+(aq) + _SCN (aq) Ag (aq) + _SCN (aq) [FeSCN]*(aq) +_ Ag+ (aq) [Ag(SCN)4] (aq) +___Fe3+ (aq) Cu'*(aq) + H2O(1) Cu²+ (aq) +_NH3(aq) [Cu(H20)4]2+(aq) + _NH3(aq) [Cu(NH3)4]?*(aq) +_H20(1) _ HNO3(aq) + _NH3(aq) __NH4OH(aq) All Co2+(aq) + _H2O(1) Co2+(aq) +_ Cl(aq) _[Co(H2O).)+(aq) +_ Cl(aq) - [CoCal” (aq) + H2O) *Side reaction
37. Balance the following equations: a. PbO2(s) —>PbO(s) + O2(g) b. Fe(OH)3(s) —>Fe2O3(s) +H2O(s) C. (NH4)2CO3(s) —>NH3(g)+H20(g) + CO2(g) d. CaCl2(aq) + H2SO4(aq) — CaSO4(s) + HCl(aq) 761
S-10 3.a) Balance the following redox equations: Ag(s) + 12(aq) Zn(s) + Cd2+ (aq) → Pb2+(aq) + I-(aq) Cd(s) + Cu2+(aq) → b) Using your calculated half-cell potentials from Question #1, calculate the standard potential for each reaction in 3.a) and identify which of these reactions are spontaneous?
Complete and balance the following equations in net ionic form and indicate the phase. 17 Zn2 NHH,O (until basic) 19. Zn2+4w" NH3(aq)(excess)→ 20 Zn2OH (until basic)-> 21. Zn(OH).(s) + OH-cao(excess) → 22. Zn2+ (m) + OH-(aq,(excess)→ (ag) (aq) Zn2+ (aq) + N产(au) + Ni(OH)2(s) + Ni2+ (aq) + 24. K+ (aq, + Fe(CN)-(ao → 25. NH, (aq, + H,00, (until basic)-→ 28, NH3(aq'(excess)→ 27, NH, (excess) 28. Ni2+ (aq) + OH-(s) → Ba2+ (aq) + SO42-(aq) → 30.
balance redox equation number 7 and 11 Cu(s) + - HNO3(aq) => Cu(NO3)2(aq) + _NO2(0) (conc, acid) Write balanced equation: 11. V + Clos (aq) => HV20, (ma) + - Cha) (basic soln.) Write balanced equation: