Question

Which of the following species is the strongest reducing agent? Mn2+ Mn Au+ H2 Au

Which of the following species is the strongest reducing agent? Mn2+ Mn Au+ H2 Au

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

reduging agent ---> is the one that will be oxidized, and reduce the other species

therefore, we need the substance easiest to oxidize (lose electrons)

Mn2+ Mn Au+ H2 Au

Buydefinition, it is always harder to strip 1 electron from a cation, therefore

Mn, H2. Au

Find potentials:

Mn2+ + 2 e− <---> Mn(s) −1.185

2 H+ + 2 e− <---> H2(g) 0.0000 = 0

Au+ + e− <---> Au(s) +1.83

From here, the easiest to oxidize is the most negative, in this case Mn2+

actually, it is easier to form Mn2O7 than to oxidize H2--> H2O or Au to AuO

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the...
Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron-transfer reaction. Mn(s) + 2Ag+(aq) Mn2+(aq) + 2Ag(s) species oxidized :------------- species reduced:---------------- oxidizing agent:----------------- reducing agent:----------------- As the reaction proceeds, electrons are transferred from------------------ to -----------------------.
Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s) +...
Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s) + 2e- ⇔ Pb(s) + 2I-(aq); E° = -0.365 V Ca2+(aq) + 2e- ⇔ Ca(s); E° = -2.868 V Pt2+(aq) + 2e- ⇔ Pt(s); E° = 1.18 V Br2(l) + 2e- ⇔ 2Br-(aq); E° = 1.066 V
Which of the following is the strongest reducing agent? Fe3+(aq) Fe2+(aq) Cd(s) F−(aq) Na(s)
Which of the following is the strongest reducing agent? Fe3+(aq) Fe2+(aq) Cd(s) F−(aq) Na(s)
Which species is the strongest oxidizing agent under standard conditions? Half-reaction Eo (V) MnO2(s) + 4H+...
Which species is the strongest oxidizing agent under standard conditions? Half-reaction Eo (V) MnO2(s) + 4H+ (aq) + 2e– → Mn2+(aq) + 2H2O(l) 1.22 V SnO2(s) + 2H2O() + 4e– → Sn(s) + 4OH– (aq) -0.95 V Hg2SO4(s) + 2e– → 2Hg(l) + SO42 – (aq) +0.61 V Cr(OH)3(s) + 3e– → Cr(s) + 3OH– (aq) –1.48 V Mn2 2+ + 2e- ⇌ Mn2 -1.18 A. MnO2 B. Sn C. Hg2SO4 D. Cr E. Mn2 2+
Consider the following half-reactions. Which of these is the strongest reducing agent listed here? I2(s) +...
Consider the following half-reactions. Which of these is the strongest reducing agent listed here? I2(s) + 2 e- → 2 I-(aq) Eo = 0.53 V S2O82-(aq) + 2 e- → 2 SO42-(aq) Eo = 2.01 V Cr2O72-(aq) + 14 H+ + 6 e- → Cr3+(aq) + 7 H2O(l) Eo = 1.33 V 1. I2(s) 2. I-(aq) 3. S2O82-(aq) 4. SO42- 5. Cr2O72- 6. Cr3+(aq)
Break down the following into: half reactions, oxidizing agent, reducing agent. 2Sr + O2? 2Sr 2Li...
Break down the following into: half reactions, oxidizing agent, reducing agent. 2Sr + O2? 2Sr 2Li + H2? 2LiH 2Cs + Br2? 2CsBr 3Mg + N2? Mg3 N2
If If an element that oxidizes easily is a strong reducing agent, wouldn't that make Tl...
If If an element that oxidizes easily is a strong reducing agent, wouldn't that make Tl the strongest reducing agent in group 3A because it can lose lose electrons easier than Al due to the fact that it is in n=6 shell versus Al which is in a n=3 shell?
which of the following species is the strongest base in an aqueous solution a) H3PO4 b)...
which of the following species is the strongest base in an aqueous solution a) H3PO4 b) H2PO4 c) HPO4^2- d) PO4^3-
Which ion is the strongest reducing agent under standard conditions? You should refer to the Eo...
Which ion is the strongest reducing agent under standard conditions? You should refer to the Eo data table. Constants Faraday constant: 9.6485 × 104 C/mol Nernst factor at 25 oC: 0.0592 V Standard Reduction Potentials (vs. SHE) Eo(Ti3+, Ti2+) = -0.90 V Eo(Zn2+, Zn) = -0.80 V (in Hg) Eo(Cr3+, Cr(s)) = -0.744 V Eo(Cr3+, Cr2+) = -0.42 V Eo(Cu2+, Cu(s)) = +0.339 V Eo(Fer3+, Fe2+) = +0.771 V Eo(Hg2+, Hg22+) = +0.908 V Cr2+ Hg22+ Ti2+ Fe2+
For each of the following reactions, identify; a. oxidized species b, reduced species c. oxidizing agent...
For each of the following reactions, identify; a. oxidized species b, reduced species c. oxidizing agent d. reducing agent 1) 2Fe(s)+3Cl2(g)----------->2FeCl3(s) 2) Mg(s)+2H2SO4(aq)--------->MgSO4(aq)+SO2(g)+2H2O(l)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT