Which of the following species can reduce Pb2+? See attached table!SRP.docx O a cu O b....
See Periodic Table See Hint The concentration of Pb2+ in a commercially available standard solution is 1.00 mg/mL. What volume of this solution should be diluted to 4.0x10 ml. to produce a solution in which the concentration of Pb2+ is 0.050 mg/L? mL
are my answers right? 6. Assuming standard conditions, indicate which of the following is true: a. H2 (g) can reduce Ag* (aq). b. H2 (g) can reduce Ni2 (aq). Falst c. Fe2 (aq) can reduce Cu (aq). Tolse - Trut d. H* (aq) can oxidize Mg(s). - True e. Pb2 (aq) can oxidize Ni(s).
Question 1 Which of the following cations is not a trace species in the human body? Zn?- Cr- Co2+ Cu- Be2-
Calculate the activity coefficient for Pb2+ at an ionic strength of 0.023 Table 6.2 Effective Diameters (az) for Selected lons lon Li Na+, IO,, HSO,, HCO,, HPO), OHT, F-, SCNT, HS, CIOj, CIO4, MnO K", cr, Br-, I-, CN-, NO2, NO, Cs+, TI+, Ag, NH: Mg+, Be2+ Ca2+, Cu2+, Zn2+, Sn2+, Mn2+, Fe2+, Ni2+, Co2 Sr2+, Ba2+, Cd+, Hg+, S2 Effective Diameter (nm) 0.9 0.6 0.45 0.35 0.3 0.25 0.8 0.6 0.5 0.45 0.40 0.9 A3, Fe3t, C3 PO, Fe(CN)...
Consider the activity series: ….. Mg > Al > Fe > Zn > H > Cu > Ag > Au …… Which of the statements will be true? i. in a voltaic cell Ag/Fe, element Ag will serve as anode and Fe will be cathode ii. Al will oxidize Cu, Ag, Au iii. Fe will reduce H, Cu and Ag iv. Cu will oxidize Al and Mg v. H is a stronger oxidizing agent than Cu, Ag A. i and...
Determine which of the following pairs of reactants will result in a spontaneous Pb2+(aq) + 2 e- - Pb(s) Eº = -0.13 V Cu+(aq) + e- - Cu(s) E = 0.52 V Ag+ (aq) + e Ag(s) Eº = 0.80 V Br2(+2 e 2 Br-(s) E° = 1.09 V reaction at 25°C. Li+(aq) + e- - Li(s) E° = -3.04 V A13+(aq) + 3 e- → Al(s) E° = -1.66 V Fe3+(aq) + 3 e" -> Fe(s) E° = -0.036...
Please help. I'm not sure how to go about figuring out which species oxidize or reduce or which are the agents. 2. Complete the table given that the following three reactions occur in the direction as written: a) 2Ag' (aq) + Fe(s) - Fe?' (aq) + 2Ag (s) b) 2Ag (aq) + Cu(s) — Cu (aq) + 2Ag (s) c) Cu (aq) + Fe (s) - Fet (aq) + Cu(s) Reaction Species oxidized Species reduced Oxidizing agent Reducing agent 3....
During a single displacement reaction, which of the following is true? The more active metal is reduced. The more active metal is oxidized. The more active metal gains electrons. The less active metal loses electrons. Which metal can reduce Pb2+? Table J: higher free metal (Fe)reacts with (1) Cu (3) Fe lower combined metal (Pb+2) (2) Hg (4) Ag
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+ #1. In the reduction table i can see several repeated values of Fe3+ one is equal to 0.77v and the second one is equal to -0.036v so, which one do I choose? Please explain. #2.If I'm asked to find the best oxidation agent, from the values already provided (Cu+, Ag+ F2 and Fe3+) which one would it be? and how would I decide from repeated values, like in #1,...
Determine the oxidation numbers of each atom in the following species H= C= C2H4 O = CO2 C= O Cu= CuO O = N = НЕ HNO3 N = NO2 N = Cu(NOs)2 Cu CraO,2 Cr= С 3 Mg = MgC2O4 O = Оз F = O = Xe ХеOFz O = H= Н202