3. a) Balance the following equation: Ag+ (aq) + Zn(s) Ag(s) + Zn2+ (aq) b) How...
Zinc metal and aqueous silver nitrate react according to the equation: Zn(s) + 2AgNO3 ---> 2Ag (s) + Zn(NO3)2 When an excess of Zn reacts with 25.00 g of AgNO3, (1.30x10^1) grams of silver are produced. What is the percent yield?
Reaction Eo Ag+(aq)+ e-→ Ag(s) 0.80V Zn2+(aq)+ 2e-→Zn(s) -0.76V What would be the cathode reactant in the Voltaic Cell made from the half-reactions above? Question options: a. Zn2+(aq) b. Ag+(aq) c. Ag(s) d. Zn(s)
Zinc metal reacts with hydrochloric acid (HCI) according to the equation: Zn(s) + 2HCl(aq) - ZnCl(aq) + H2(g) Part A How many grams of hydrogen are produced if 300 g of zinc reacts? AEP O ? M . Submit Request Answer
how do these things affect eachother? if I have Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) and the solution in the salt bridge is changes to CH3OH from potassium nitrate. if I have Fe3+(aq)|Fe2+(aq)||Ag+(aq)|Ag(s) and the iron (ii) nitrate solution is replaced with salt water if I have Cu(s)|Cu2+(aq)||MnO4^-(aq)|C(s) and I replaced the carbon electrode with silver the rest are voltaic cells if I have Co (s) | Co2+ (aq)|| Cu2+(aq) |Cu (s) instead of a porous cup we turn it into two half cells connected...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E = 0.799 V Determine the voltage of the galvanic cell generated from these two half reactions, and calculate E of the cell when Zn2+ (aq) = 0.0100 M and Ag+ (aq) = 0.900 M at 25°C. Report the value of E
Balance each of the following skeletal equations: (a) Mg(s)+ O2(g) (b) Zn(s)+ AgNO3(aq) Zn(NO3)2(aq) + Ag(s) (c) C2H2(g)+O2(g) CO2(g) + H20(g) 5.38 MgO(s) odm(d) C12H22O11(s) +KCIO3(I) Constder the foll CO2(g) +H20(g) + KCI(s)
According to the reaction below, how many grams of zinc, Zn, could react in 151.46 mL of 1.084 M AgNO3? Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq)
According to the reaction below, how many grams of zinc, Zn, could react in 147.96 mL of 1.778 M AgNO3? Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq)
Consider the unbalanced redox reaction: MnO−4(aq)+Zn(s)→Mn2+(aq)+Zn2+(aq) Balance the equation in acidic solution. Part B- Determine the volume of a 0.475 M KMnO4 solution required to completely react with 3.35 g of Zn.
For a silver-zinc voltaic cell containing Ag+(aq) and Zn2+(aq) solutions, do the following. (a) Identify the cathode. (Include states-of-matter under the given conditions in your answer. Type INERT if an inert electrode must be used.) (b) Identify the half-reaction that occurs at the cathode. (Include states-of-matter under the given conditions in your answer.)