Calculate AG for the following reaction: Mn (s) + Zn²+ (aq) → Mn²" (aq) + Zn (s) 0-8. 10 x 101 J O-4. 10 x 10 J +3.74 x 10 J

Balance the following redox reaction in acidic solution. 2+ Fe²+ (aq) + MnO₂(s) ->> 3+ 2+ Fe (aq) +Mn (aq)

Balance the reaction of copper plus nitrate to yield copper (II) and nitrogen dioxide.  This reaction occurs in acidic solution.     Cu  +  NO3-   ------->    Cu2+   +   NO2     Cu(NO3)2   +  4 H+-------->  Cu   +   2 NO2   +   2 H2O     2 Cu2+   +   4 H2O   +   2 NO2  -------->  Cu   +   2 NO3-   +   8 H+     10 HCl   +   5 Cu   +   2 NaNO3  -------->   5 CuCl2   +   2 NaNO2   +   2 H2O     Cu   +   4 H+   +   2 NO3-  -------->  Cu2+   +   2 NO2   +   2 H2O

Write the equilibrium constant expression for this reaction: 2Li*(aq) +Co (aq) Li,CO,(s) X log, cos, K =

Calculate the standard free‑energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this table.   2Au3+(aq)+3Ni(s)↽−−⇀2Au(s)+3Ni2+(aq) Δ?∘=   kJ/mol

Using data in the Table, what is the equilibrium constant for the reaction: 2Fe 3+(aq)+H 2(g) 2Fe 2+(aq) + 2H +(aq)?

Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu²+ (aq) + Pb(s) → Cu(s) + Pb²+ (aq) 2+ Cu²+ (aq) + 2e Pb²+ (aq) + 2e → Cu(s) Fre 0.337 V → Pb(s) Fe -0.126 V red = Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be | than zero.

Balance the redox reaction in acidic solution:Cu(s)+NO−3(aq)→Cu2+(aq)+NO2(g) Express your answer as a chemical equation including phases.

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu²+ (aq) + 2Cu+ (aq) → Cu(s) + 2Cu²+ (aq) 2+ Cu²+ (aq) + 2e → Cu(s) Ee = 0.337 V red 0.153 V = 2+ Cu²+ (aq) +e → Cut (aq) E red AG° kJ K for this reaction would be than one.

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.