Will H2O2 ever be a viable automotive fuel?

I heard about a car the other day that runs on Hydrogen Peroxide (H2O2). Its only emission is water vapor and oxygen, which sounds cool, but then I looked into it a bit more and I don’t see any viability coming from it and wanted to know what others think of it.

First concern is price. Currently the car in question runs off of a 50% solution! The stuff in the drug stores is only 3%! 50% runs about $120 a gallon which seems really expensive. Also it isn’t that easily accessible. I would think any fuel station would be expensive to build and that cost would be added to the consumer. H2O2 is a corrosive agent and can’t be stored in steel drums IIRC. I know that the most common way to make Hydrogen Peroxide is through the use of electricity. This is really ineffective as you can never get back out all the energy put into it.

Second concern is safety. The emission is not water vapor at the pure form – it is super heated steam! I could see this causing severe burns if not death to anyone too close to the exhaust. Also with the massive amount of water vapor, I can’t see any normal exhaust system holding up to the abuse over any number of years as most normal exhaust system would just rust away.

H2O2 is widely used in rockets, and even some underwater applications because it doesn’t require oxygen to produce thrust as its oxidation process produces a lot of volume. Even so, it is still very expensive for these uses. With the electric and hybrid cars being more commonplace, is there even a reason to explore the use of H2O2 in practical everyday automobile use??

Can lack of oxygen at birth cause developmental delays?

My son had lack of oxygen and need oxygen of two days, now he is 4 and has issues.Does anyone have experience with this. Has your kid got better with therapy?

H2O2+MnO2= What is the decomposition reaction??

HW HELP PLSSSSS! Chemistry sucks ?

16) name each of the binary molecular compounds in item 11 using the stock system.

26) name each of the following ionic compounds using the Stock system:
a. NaCl
b. KF
c. CaS
d. CO(NO3)2
e. FePO4
f. Hg2SO4
g. Hg3(PO4)2

48) assign oxidation numbers to each atom in the following molecules and ions:
a. CO2
b. NH^+4
c. MnO^-4
d. S2O^-2 3
e. H2O2
f. P4O10
g. OF2

**more chemitsry questions!!**?

1) Given:
2 MnO4- + 5 H2O2 + 6 H+2 Mn+2 + 8 H2O + 5 O2

What volume of a 0.150M KMnO4 solution would be needed to titrate 75.0mL of a 0.150M H2O2 solution?
45.0 mL
75.0 mL
15.0 mL
30.0 mL
none of these

2)Which one of the following is a redox reaction?
H+ (aq) + OH- (aq)3H2 + AlCl3
CO32- (aq) + HSO4- (aqHCO3- (aq) + SO42- (aq)
2KBr(aq) + Pb(NO3)2 (aq) 2KNO3 (aq) + PbBr2 (s)
CaBr2 (aq) + H2SO4 (aq)CaSO4 (s) + 2HBr(g)
2Al(s) + 3H2SO4 (aq) Al2(SO4)3 (aq) + 3H2 (g)

3) What are the respective oxidation numbers of sulfur in the thiosulfate ion (S2O32-) and the tetrathionate ion (S4O62-)?
-2, -2.5
+2, +2.5
+0.5, +1
+3, +3
-0.5, -1

4) What volume of 12.0M nitric acid is required to prepare 6.00 L of 0.100 M nitric acid?
0.05 L
0.50 L
1.0 L
0.02 L
1.20 L

5) The electron dot formula for AsCl3 shows:
two single bonds, one double bond, and 9 lone pairs
a total of 84 electron dots
one single bond, two double bonds, and 8 lone pairs
three single bonds and 10 lone pairs
three single bonds and one lone pair

Assign oxidation numbers to all elements in each compound or ion below:?

1.HCl
2.KNO3
3.OH-
4.Mg3N2
5.KClO3
6.Al(NO3)3
7.S8
8.H2O2
9.PbO2
10.NaHSO4
11.H2SO3
12.H2SO4
13.BaO2
14.KMnO4
15.LiH
16.MnO2
17OF2
18.SO3
19.NH3
20.Na

5 Electrochemistry questions…?

1. Cr2O7^2- + 6I^- + 14 H^+ –> 2Cr^3+ + 3I2 + 7H2O
Which of the following statements about the reaction given above is NOT true?
A) The oxidation number of chromium changes from +6 to +3.
B) The oxidation number of iodine changes from -1 to 0.
C) The oxidation number of hydrogen changes from + 1 to 0.
D) The oxidation number of oxygen remains the same.
E) The reaction takes place in acidic solution.

2. Al^3+ + 3e^- –> AI(s)
Eº = -1.66 V
Cr^3+ + 3e^- –> Cr(s)
Eº = -0.74 V
The standard reduction potentials for two half-reactions are shown above. Which of the statements listed below will be true for the following reaction taking place under standard conditions?
AI(s) + Cr^3+ –> Al^3+ + Cr(s)
A) Eº = 2.40 V, and the reaction is not spontaneous.
B) Eº = 0.92 V, and the reaction is spontaneous.
C) Eº = -0.92 V, and the reaction is not spontaneous.
D) Eº = -0.92 V, and the reaction is spontaneous.
E) Eº = -2.40 V, and the reaction is not spontaneous.

3.In which of the following molecules does hydrogen have an oxidation state of -1?
A) HP
B) NH3
C) CaH2
D) CH4
E) H2

4.The equation for the decomposition of H2O2 is shown below.
2H2O2 –> 2H2 + O2
Which of the following statements about the reaction shown above is true?
A) Oxygen is reduced, and hydrogen is oxidized.
B) Oxygen is oxidized, and hydrogen is reduced.
C) Oxygen is both oxidized and reduced.
D) Hydrogen is both oxidized and reduced.
E) Neither oxygen nor hydrogen change oxidation state.

5.When solid iron is brought into contact with water and oxygen, it undergoes the following half-reaction:
Fe(s) –> Fe^2+(aq)
This half-reaction is instrumental in the corrosion of iron. When iron is coated with solid zinc, the half-reaction above is impeded, even if the zinc coating is incomplete. This is most likely because
A) Zn(s) is more easily reduced than Fe(s).
B) Zn(s) is more easily oxidized than Fe(s).
C) Zn^2+(aq) is more easily reduced than Fe(s).
D) Zn^2+(aq) is more easily oxidized than Fe(s).
E) Zn(s) is more easily reduced than Fe^2+(aq).

Thank you for helping me!!! I really do appreciate it! If it won’t steal your time too much, could you explain these and how you got the answers too? Thanks!

What are the oxidation numbers for the elements in these compounds?

What are the oxidation numbers for the elements in the compounds below:

1) H2O

2) H2O2

3) ClO3-

4) Pb3(PO4)4

How can oxygen in the body influence a cell’s polarity and a field or its gravitational forces in the body?

Hyperoxigenation therapy has to do with medicine (it is an alternative treatment where one is administered high doses of intravenous O2 – i think in the form of o3). Since the body operates on biophysics, there must be an association between oxygen and how it can alter magnetic fields, gravitational forces and such, which then helps to explain part of the therapy‘s success still unrecognized. On the long run, this is to illustrate myself and others the importance of breathing and how the lack of it can lead to a disrupted cell environment and communication (in terms of its “field”). Any hints or references please.

Can someone check these ten questions and tell me how to do the ones I missed. Really struggled with these.?

2) State the oxidation number for each of the following nonmetals.
a) H2
b) He
c) P4
d) I2
a) 0
b) 0
c) 0
d) 0

10) Supply the term that corresponds to each of the following.
a) a substance that increases its oxidation number in a redox reaction
b) a substance that decreases its oxidation number in a redox reaction
a) Oxidizing agent
b) Reducing agent

14) Indicate the oxidizing and reducing agents in the following redox reactions.
a) Ca(s) + 2 H2O(l) ? Ca(OH)2(aq) + H2(g)
b) Mg(s) + 2 HCl(aq) ? MgCl2(aq) + H2(g)
a) Ca is the reducing agent and H2 is the oxidizing agent
b) Mg is the reducing agent and H2 is the oxidizing agent

24) Write a balanced equation for each of the following redox reactions using the oxidation number method.
a) Fe2+(aq) + H2O2(aq) + H+(aq) ? Fe3+(aq) + H2O(l)
b) Cr2O72-(aq) + Br-(aq) + H+(aq) ? Cr3+(aq) + Br2(l) + H2O(l)
a) 2 Fe2+(aq) + H2O2(aq) + 2 H+(aq) ? 2 Fe3+(aq) + 2 H2O(l)
b) Cr2O72-(aq) + 6 Br-(aq) + 14 H+(aq) ? 2 Cr3+(aq) + 3 Br2(l) + 7 H2O(l)

36) Sulfur can undergo a redox reaction in which it is simultaneously oxidized and reduced. Write a balanced equation for the following in a basic solution.
S(s) ? SO32-(aq) + S2-(aq)
3 S(s) + 6 OH- ? SO32-(aq) + 2 S2-(aq) + 3 H2O(l)

40) Refer to Table 17.3 and indicate which substance in each of the following pairs is the stronger reducing agent.
a) Cu(s) or Cr(s)
b) H2(g) or Cu(s)
c) Cu(s) or I-(aq)
d) Cl-(aq) or H2(g)
a) Cr(s)
b) H2(g)
c) Cu

54) The spontaneous redox reaction of hydrogen gas and iodine occurs according to the following equation.
H2(g) + I2(s) ? 2 H+(aq) + 2 I-(aq)
Assume the half-reactions are separated into two compartments. A hydrogen gas Pt electrode is immersed in 1.00 M HI, and a second Pt electrode is placed in 1.00 M KI-I2 solution. Indicate each of the following in this voltaic cell.
a) oxidation half-cell reaction
b) reduction half-cell reaction
c) anode and cathode
d) direction of electron flow
e) direction of I- in the salt bridge
a) H2 ? H+ + 1 e-
b) I2 + 1 e- ? I-
c) H2 is the anode because it is where the oxidation occurs and I2 is the cathode because it is where reduction occurs.
d) Electrons flow from H2 anode to I2 cathode
e) I- flow from the I2 cathode towards the H2 anode

60) The nonspontaneous redox reaction of lead and zinc nitrate solution occurs according to the following ionic equation.
Pb(s) + Zn2+(aq) ? Zn(s) + Pb2+(aq)
Assume the half-reactions are separated into two compartments. A zinc electrode is immersed in 1.00 M , Zn(NO3)2 and a lead electrode in 1.00 M Pb(NO3)2. Indicate each of the following in this electolytic cell.
a) oxidation half-cell reaction
b) reduction half-cell reaction
c) anode and cathode
d) direction of electron flow
e) direction of NO3- in the salt bridge
a) Pb ? Pb2+ + 2 e-
b) Zn2+ + 2 e- ? Zn
c) Pb is the anode and Zn is the cathode
d) Electrons flow from Pb anode to Zn cathode
e) NO3- flows from the Zn cathode towards the Pb anode

66) The redox reaction between liguid mercury and aqueous gold(III) acetate produces mercury(I) acetate and gold metal. Write a net ionic equation for this reaction.
3 Hg(l) + 2 Au(O2CCH3)3(aq) ? 3 Hg(O2CCH3)2(aq) + 2 Au(s)

70) Write a balanced equation for the reaction of ethyl alcohol, C2H5OH, and acidic potassium dichromate solution.
C2H5OH(aq) + Cr2O72-(aq) ? HC2H3O2(aq) + Cr3+(aq) + H2O(l)
3 C2H5OH(aq) + 2 Cr2O72-(aq) + 16 H+ ? 3 HC2H3O2(aq) + 4 Cr3+(aq) + 11 H2O(l)