Calculate Ho for the following equations:
a. Zn(s) + 2H+(aq) Zn2+(aq) + H2(g)
b. 2H2S(g) + 3O2(g) 2SO2(g) + 2H2O(g)
c. 3Ni(s) + 2NO3-(aq) + 8H+(aq) 3Ni2+(aq) + 2NO(g) + 4H2O(l)
Calculate Ho for the following equations: a. Zn(s) + 2H+(aq) Zn2+(aq) + H2(g)&n
For a voltaic cell based on the reaction below, which statement is correct? Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) Zn2+(aq) is oxidized at the anode. H+(aq) is reduced at the cathode. Zn2+(aq) is reduced at the anode. H2(g) is the oxidizing agent.
Question 1 1 pts For the cell: Zn(s) + 2H+ (aq) + Zn2+(aq) + H2 (g) If [Zn2+) = 1 M, PH2 = 1 atm, and E = 0.549 V what is pH? Question 2 1 pts Calculate the voltage for the following cell at 25° ZnZn+2 ( 2.832 M) || Cd2+ (0.027 M)| Cd
reaction. oxung H Zn(s) + 2H*(aq) — Zn2+ (aq) + H2(g) Reducing Agent - 2n 10. When 1.00 L of a water sample was treated with excess Ba2+ ions, 4.00 g of BaCO3 was formed. What mass of carbonate ions was present in the original 1.00-L sample? holar mass Bacon -197.39 /mol 4.00 g of BaCO3 = 4.00/197.34 mol 133 11. Complete each of the following reactions: a. Ag +LiNO - Ao V03 law) 7 03) b. Zn + Cu(NO3),...
Calculate the equilibrium constant for each of the reactions at 25 ∘C. a. 2Cr3+(aq)+3Sn(s)→2Cr(s)+3Sn2+(aq) b. O2(g)+2H2O(l)+2Sn2+(aq)→4OH−(aq)+2Sn4+(aq) c. 2Cr3+(aq)+3Ni(s)→2Cr(s)+3Ni2+(aq)
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)
1. Consider the reaction below: 3Ag2S(s) + 8H+(aq) + 2NO3-(aq) ? 6Ag+(aq) + 3S(s) + 2NO(g) + 4H2O(l) In this reaction, which species is reduced? 2. Calculate Ecell for the following electrochemical cell which is operating under nonstandard conditions: Cr | Cr3+(0.010 M) || Ag+(0.00010 M) | Ag The relevant standard reduction potentials are: Cr3+(aq) + 3e- ? Cr(s) Eº = ?0.74 V Ag+(aq) + e- ? Ag(s) Eº = +0.80 V
Classify the half‑reactions as reduction half‑reactions or oxidation half‑reactions. H2(g)⟶2H+(aq)+2e−H2(g)⟶2H+(aq)+2e− 12O2(g)+2H+(aq)+2e−⟶H2O(g)12O2(g)+2H+(aq)+2e−⟶H2O(g) Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e−Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e− 2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq)2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq) Fe(s)⟶Fe2+(aq)+2e−Fe(s)⟶Fe2+(aq)+2e− oxidation reduction reduction oxidation reduction
Which of the following reactions corresponds to the thermochemical equation for the standard molar enthalpy of formation of solid zinc nitrate? a. Zn(s) + 2N(g) + 6O(g) → Zn(NO3)2(s) b. Zn(s) + 2HNO3(aq) → Zn(NO3)2(s) + H2(g) c. Zn(OH)2(s) + 2HNO3(aq) → Zn(NO3)2(s) + 2H2O() d. Zn2+(aq) + 2NO3–(aq) → Zn(NO3)2(s) e. Zn(s) + N2(g) + 3O2(g) → Zn(NO3)2(s)
(2 pts.) For the following electrochemical cell at 25°C: Zn(s) | Zn2+ (aq) || H+ (aq) | Pt,H2 (g) (P=1.00 atm) calculate DG° in kJ calculate Ecell for [H+] = 0.8 M and [Zn2+] = 0.5 M calculate K at 25°C
According to the equation: Zn(s) + 2HCl(aq) ----> H2(g) + ZnCl(aq), calculate the volume (L) of H2 gas that can be formed at 25 °C and a pressure of 854 mmHg when 25.0 g of Zn is used in the reaction.