Hello, Just in need of a little help understanding a spontaneous and non-spontaneous redox reaction spontaneous...
Hello,
Just in need of a little help understanding a spontaneous and non-spontaneous redox reaction
spontaneous redox reaction for a battery is Pb(s) +PbO2(s) +SO4(aq) = PbSO4. Does that mean that the non-spontaneous, reverse reaction that occurs and re-charges the battery is PbSO4(s) = Pb(s) + PbO2(S) +SO4(aq)
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Hello,
Just in need of a little help understanding a spontaneous and
non-spontaneous redox reaction
spontaneous...
Need help with questions 1-5 D Determine whether each redox reaction occurs spontane- ously in the...
Need help with questions 1-5
D Determine whether each redox reaction occurs spontane- ously in the forward direction. (a) Ca2+(aq) + Zn(s)-Ca(s) + Zr"(al) (b) 2 Ag+(aq) + Ni(s)--2 Ag(s) + N产(aq) (c) Fe(s) +Mn2 (aą)- Fe (aą)Mn(s) (d) 2 Al(s) + 3 Pb2+(aq) → 2 AP"(aq) + 3 Pb(s) Suppose you wanted to cause Pb ions to come out of solu- tion as solid Pb. What metal could you use to accomplish this? Make a sketch of an electrochemical...
I really need some help with number 7 and number 8. I really appreciate the help!...
I really need some help with number 7 and number 8. I
really appreciate the help!
c. CuCl2 f. HSO4- Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. 4 Li (s) + O2 (g) → 2 Li20 (s) b. Mg (s) + Fe2+ (aq) → Mg2+ (aq) + Fe (s) c. Pb(NO3)2 (aq) + Na2SO4 (aq) → PbSO4 (s) + 2 NaNO3 (aq) d. HBr (aq) +...
need help with these 2 please asap Which of the following reactions is a non-redox reaction?...
need help with these 2 please asap
Which of the following reactions is a non-redox reaction? O 2 H, 02H2 + O2 O2KCIO3 -- 2KCI + 3 02 o CaO + H2O = Ca(OH)2 O 2 SO2 + 02 - 2 SO, Question 42 2 pts Which substance functions as a oxidizing agent in the following redox reaction? CH4 + 20 C0, + 2H2O H20 CO2 CHA
I just need some help on how to start off balancing the equations for both questions....
I just need some help on how to start off balancing
the equations for both questions.
J. Muench Group Activity #10 CHEM 162 1. Balance the following redox reactions that occur in acidic solutions. a. Asis) + SO4 (aq) → AsO4 (aq) + SO218) b. Craq) + Bio-ag) → Cr20; aq) + Bilaq)
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
i need help answering these qoustions plz?????? Based on the solubility rules given in class, classify...
i need help answering these qoustions plz??????
Based on the solubility rules given in class, classify the following compounds as solid (s) or aqueous (aq) when added to water: a) Al(OH)3 b) Li3PO4 c) BaSO4 d) (NH4)2CO3 c) Mg(ClO3)2 f) HgCl2 Which combination of reactants results in an acid/base neutralization reaction? a. HNO3(aq) + Zn(s) → b. Mg(C104)2(aq) + NaOH(aq) → c. Ca(s) + H2SO4(aq) - d. H2CO3(aq) + LiOH(aq) → CA OB C What is the net ionic equation...
Chem 1212 Lab Report on electrochemistry Electrochemistry When electrons transfer between reaction components in a redox...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - &
1. Which of the following conditions defines a non-spontaneous oxidation-reduction reaction? E° + ΔG° - Keq <1 E° - ΔG° - Keq <1 E° + ΔG°+ Keq >1 E° + ΔG°- Keq >1 E° - ΔG° + Keq <1 2. What information can be obtained from the Figure below? The equivalence point occurs at pH = 7.0 but the pKa is not known from the graph. Both the pOH and the...
I need help with questione 1-12 and discussion question 1 and 2. The previous pictures help...
I need help with questione 1-12 and discussion question 1 and
2. The previous pictures help determine the chart. Please Show Work
thank you so much
An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
I really need help understanding this question, especially the formal charge, I just don't get what...
I really need help understanding this question, especially the formal charge, I just don't get what I am doing wrong. Draw Kekulé structures for each compound. Indicate all formal charges CH3CHCHCH2Cl CH3C(CH3)2 CHO BF3 HN3
Need help with questions 1-5
D Determine whether each redox reaction occurs spontane- ously in the forward direction. (a) Ca2+(aq) + Zn(s)-Ca(s) + Zr"(al) (b) 2 Ag+(aq) + Ni(s)--2 Ag(s) + N产(aq) (c) Fe(s) +Mn2 (aą)- Fe (aą)Mn(s) (d) 2 Al(s) + 3 Pb2+(aq) → 2 AP"(aq) + 3 Pb(s) Suppose you wanted to cause Pb ions to come out of solu- tion as solid Pb. What metal could you use to accomplish this? Make a sketch of an electrochemical...
I really need some help with number 7 and number 8. I
really appreciate the help!
c. CuCl2 f. HSO4- Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. 4 Li (s) + O2 (g) → 2 Li20 (s) b. Mg (s) + Fe2+ (aq) → Mg2+ (aq) + Fe (s) c. Pb(NO3)2 (aq) + Na2SO4 (aq) → PbSO4 (s) + 2 NaNO3 (aq) d. HBr (aq) +...
need help with these 2 please asap
Which of the following reactions is a non-redox reaction? O 2 H, 02H2 + O2 O2KCIO3 -- 2KCI + 3 02 o CaO + H2O = Ca(OH)2 O 2 SO2 + 02 - 2 SO, Question 42 2 pts Which substance functions as a oxidizing agent in the following redox reaction? CH4 + 20 C0, + 2H2O H20 CO2 CHA
I just need some help on how to start off balancing
the equations for both questions.
J. Muench Group Activity #10 CHEM 162 1. Balance the following redox reactions that occur in acidic solutions. a. Asis) + SO4 (aq) → AsO4 (aq) + SO218) b. Craq) + Bio-ag) → Cr20; aq) + Bilaq)
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
i need help answering these qoustions plz??????
Based on the solubility rules given in class, classify the following compounds as solid (s) or aqueous (aq) when added to water: a) Al(OH)3 b) Li3PO4 c) BaSO4 d) (NH4)2CO3 c) Mg(ClO3)2 f) HgCl2 Which combination of reactants results in an acid/base neutralization reaction? a. HNO3(aq) + Zn(s) → b. Mg(C104)2(aq) + NaOH(aq) → c. Ca(s) + H2SO4(aq) - d. H2CO3(aq) + LiOH(aq) → CA OB C What is the net ionic equation...
Chem 1212 Lab Report on electrochemistry
Electrochemistry When electrons transfer between reaction components in a redox reaction, we can harness the motion of the electrons to create a potential. Electrochemistry revolves around the separation of the two half-reactions in a redox reaction and establishing two different electrodes. This might involve physically separating the half-reactions or including a separator, such as a semi-permeable membrane or plastic dividers. With the reactions separated, the electrons will need to flow through the wire connecting...
I need help with questione 1-12 and discussion question 1 and
2. The previous pictures help determine the chart. Please Show Work
thank you so much
An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
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