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Chemguide - questions REDOX EQUATIONS 1. Use each of the following pairs of electron-half-equations to work...
3. Calculate the redox potential (in volts) for a LiMnO2/graphite battery. (Redox reaction) MnO4- + 8H...
3. Calculate the redox potential (in volts) for a
LiMnO2/graphite battery.
(Redox reaction)
MnO4- + 8H + 5e- →
Mn2+ (aq) + 4H2O (+1.51 V)
MnO2 + 4H +2e-
→ Mn2+ (aq) + 2H2O (+1.22 V)
xLi+ + C6 + e- → LixC5 (-3.00
V)
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f....
3. Calculate the redox potential (in volts) for a LiMnO2/graphite battery. MnO4- + 8H + 5e-...
3. Calculate the redox potential (in volts) for a
LiMnO2/graphite battery.
MnO4- + 8H + 5e- →
Mn2+ (aq) + 4H2O (+1.51 V)
MnO2 + 4H +2e-
→ Mn2+ (aq) + 2H2O (+1.22 V)
xLi+ + C6 +
e- → LixC5 (-3.00 V)
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The reaction...
1. Write balanced equations for the following processes. a. The reaction of potassium with water. c....
1. Write balanced equations for the following processes.
a. The reaction of potassium with water.
c. Thermal decomposition of sodium azide.
d. The reaction of potassium peroxide with water.
e. Calcium hydride reacting with water.
f. The reaction between ethanol and lithium hydride.
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The...
1. Write balanced equations for the following processes. a. The reaction of potassium with water. c....
1. Write balanced equations for the following processes.
a. The reaction of potassium with water.
c. Thermal decomposition of sodium azide.
d. The reaction of potassium peroxide with water.
e. Calcium hydride reacting with water.
f. The reaction between ethanol and lithium hydride.
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The...
1. How do I read the half reaction table? 2. If im asked for the best...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
2. What are products of the following reaction? (note: the reactants are not necessarily balanced) KO2...
2. What are products of the following reaction? (note: the
reactants are not necessarily balanced)
KO2 + H2O → ________ + __________
NaHCO3 + heat → ________ + ________ + ________
NaNH2 + H2O → ________ + ________
LiC4H9 + C2H5OH →
________ + ________
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water....
For all of the following experiments, under standard conditions, which species could be spontaneously produced? A...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+ #1. In the reduction table...
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,...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
Sodium metal is prepared by electrolysis of sodium chloride to the metal and chlorine gas. Using the...
Sodium metal is prepared by electrolysis of sodium
chloride to the metal and chlorine gas. Using the
reduction potentials attached, calculate E° and ΔG° for the overall
reaction.
TABLE 12.2 Standard Reduction Potentials at 25°C Half-reaction Eº, V Increasing strength as oxidizing agent Lit(aq) + e Li(s) K+(aq) + e → KS) Ba2+ (aq) + 2e → Ba(s) Sr2+(aq) + 2e → Sr(s) Ca2+(aq) + 2e → Ca(s) Na*(aq) + e Na(s) Mg2+ (aq) + 2e → Mg(s) Be2+(aq) + 2e...
3. Calculate the redox potential (in volts) for a
LiMnO2/graphite battery.
(Redox reaction)
MnO4- + 8H + 5e- →
Mn2+ (aq) + 4H2O (+1.51 V)
MnO2 + 4H +2e-
→ Mn2+ (aq) + 2H2O (+1.22 V)
xLi+ + C6 + e- → LixC5 (-3.00
V)
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f....
3. Calculate the redox potential (in volts) for a
LiMnO2/graphite battery.
MnO4- + 8H + 5e- →
Mn2+ (aq) + 4H2O (+1.51 V)
MnO2 + 4H +2e-
→ Mn2+ (aq) + 2H2O (+1.22 V)
xLi+ + C6 +
e- → LixC5 (-3.00 V)
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The reaction...
1. Write balanced equations for the following processes.
a. The reaction of potassium with water.
c. Thermal decomposition of sodium azide.
d. The reaction of potassium peroxide with water.
e. Calcium hydride reacting with water.
f. The reaction between ethanol and lithium hydride.
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The...
1. Write balanced equations for the following processes.
a. The reaction of potassium with water.
c. Thermal decomposition of sodium azide.
d. The reaction of potassium peroxide with water.
e. Calcium hydride reacting with water.
f. The reaction between ethanol and lithium hydride.
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f. The...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
2. What are products of the following reaction? (note: the
reactants are not necessarily balanced)
KO2 + H2O → ________ + __________
NaHCO3 + heat → ________ + ________ + ________
NaNH2 + H2O → ________ + ________
LiC4H9 + C2H5OH →
________ + ________
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water....
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
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,...
Use the galvanic cell notation to describe the Daniell cell. (4 marks) Using the reduction potential table calculate Eº for the Daniel cell. 12 marks) Calculate the equilibrium constant K for the reaction Cu2+ + Zn → Cu + Zn²+, at 25 °C. (4 marks) Standard Potentials at 25°C Half Reaction Potential Potential +2.87 V 0.000 V +2.07 V -0.04 V +2.05 V -0.13 V -1.69 V -0.14 V +1.69 V -0.23 V +1.67 V -0.26 V +1.63 v -0.28...
Sodium metal is prepared by electrolysis of sodium
chloride to the metal and chlorine gas. Using the
reduction potentials attached, calculate E° and ΔG° for the overall
reaction.
TABLE 12.2 Standard Reduction Potentials at 25°C Half-reaction Eº, V Increasing strength as oxidizing agent Lit(aq) + e Li(s) K+(aq) + e → KS) Ba2+ (aq) + 2e → Ba(s) Sr2+(aq) + 2e → Sr(s) Ca2+(aq) + 2e → Ca(s) Na*(aq) + e Na(s) Mg2+ (aq) + 2e → Mg(s) Be2+(aq) + 2e...
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