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consider the solubility of a mineral. It is a FeS(s) mineral.
S is -2 oxidation state....
consider the solubility of a mineral. It is a FeS(s) mineral. S is -2 oxidation state....
consider the solubility of a mineral. It is a FeS(s) mineral.
S is -2 oxidation state. The mineral is found in a mud solution,
see the following chemical equation which is under equilibrium in
the atmosphere.
1) find the oxidation state of S, Fe, and H in each species of
the balance. is it an oxidation-reduction reaction?
2) If the condition is at 25 degrees C, pH=4.2, Fe2+
concentration is 4 ppm, and logK= 3.0. What is the partial pressure...
2. Label each element with its oxidation state, use arrows to identify the reduction and oxidation, and balance the following redox reaction, which takes place under basic conditions. Please draw a b...
2. Label each element with its oxidation state, use arrows to identify the reduction and oxidation, and balance the following redox reaction, which takes place under basic conditions. Please draw a box around your final balanced equation. [Note: this is a disproportionation reaction in which a species (e.g., P is oxidized and reduced.] P4 (s)PH (g) +HPO,2(aq)
2. Label each element with its oxidation state, use arrows to identify the reduction and oxidation, and balance the following redox reaction, which...
Consider the unbalanced chemical reaction shown below: Cu(s)+HNO3(aq)→Cu(NO3)2(aq)+NO(g)+H2O(l) The oxidation state of Cu in Cu(s)Cu(s) =...
Consider the unbalanced chemical reaction shown below: Cu(s)+HNO3(aq)→Cu(NO3)2(aq)+NO(g)+H2O(l) The oxidation state of Cu in Cu(s)Cu(s) = The oxidation state of Cu in Cu(NO_3)_2(aq)Cu(NO3)2(aq) = The oxidation state of N in HNO_3(aq)HNO3(aq) = The oxidation state of N in NO(g)NO(g) = The total number of electrons transferred in this reaction is = The sum of the coefficients in the balanced chemical reaction =
7. A low concentration of NTA has equilibrated with PbCO3(s) at pH 7.00 in a medium...
7. A low concentration of NTA has equilibrated with
PbCO3(s) at pH 7.00 in a medium having a final
HCO3- concentration of 7.50x10-4
M.
a. Determine [Pb2+].
b. Write out KT and the overall reaction for
KT.
c. What is the ratio of [Pb(NTA)- ] to
[H(NTA)2-] in this solution?
Potentially useful data: Reaction Hg 2 +2e = Hgº(s) Feste = Fe2 Cu 2 +2e = Cuº(s) 2H + 2e = H2(g) Pb2 +2e=Pbº(s) Ca*2 + 2e = Cdº(s) 1/4...
8. Sodium bicarbonate, NaHCO3, undergoes thermal decomposition according to the reaction: 2 NaHCO3 (s) + Na2CO3...
8. Sodium bicarbonate, NaHCO3, undergoes thermal decomposition according to the reaction: 2 NaHCO3 (s) + Na2CO3 (s) + CO2 (g) + H20 (g). How does the equilibrium position shift as a result of each of the following disturbances? a. 0.20 atm argon is added. b. NaHCO3 (s) is added. c. Mg(CIO)2 is added as a drying agent to remove H2O vapor. d. Dry ice (Solid CO2) is added. e. The volume of the container decreases. f. The temperature of the...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....
8. Using the Nernst equation, determine the ratio of Hg2+ to Cu2+ at equilibrium in an electrochemical cell in otherwise...
8. Using the Nernst equation, determine the ratio of
Hg2+ to Cu2+ at equilibrium in an
electrochemical cell in otherwise pure water, when in contact with
Hg(s) and Cu (s)
Potentially useful data: Reaction Hg 2 +2e = Hgº(s) Feste = Fe2 Cu 2 +2e = Cuº(s) 2H + 2e = H2(g) Pb2 +2e=Pbº(s) Ca*2 + 2e = Cdº(s) 1/4 O2(g) + H + = 1/2 H2O 2 02(g) + 2H+ + 2e = H,O2 1/2 NO3 + H +...
6. Given a total dissolved lead concentration of 2.0x10-5 M, a total dissolved NTA concentration of...
6. Given a total dissolved lead concentration of
2.0x10-5 M, a total dissolved NTA concentration of
2.0x10-2 M, and a pH of 12.3 (note extreme pH)
a. Under these conditions, what is the dominant form of NTA?
b. Write an equation for total dissolved NTA and for total
dissolved Pb. What assumptions can you make?
c. Calculate the predicted [Pb2+], considering NTA
complexation only?
d. What is the [Pb2+] as predicted by the solubility
of Pb(OH)2(s) at pH 12.3?
e....
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
When answering Parts a-h, consider only the molecules and ions, Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq), and Cr2O7^2-(aq), under standard state conditions. (1 pt each) Use standard reduction...
When answering Parts a-h, consider only the molecules and ions,
Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq),
and Cr2O7^2-(aq), under standard state conditions. (1 pt each)
Use standard reduction table.
a) Which of these molecules and ions are oxidizing agents?
b) Which of these molecules and ions are reducing agents?
c) List the oxidizing agents from part a in DECREASING order of
oxidizing agent strength. (strongest OA to weakest OA)
d) List the reducing agents from part b in DECREASING order of...
consider the solubility of a mineral. It is a FeS(s) mineral.
S is -2 oxidation state. The mineral is found in a mud solution,
see the following chemical equation which is under equilibrium in
the atmosphere.
1) find the oxidation state of S, Fe, and H in each species of
the balance. is it an oxidation-reduction reaction?
2) If the condition is at 25 degrees C, pH=4.2, Fe2+
concentration is 4 ppm, and logK= 3.0. What is the partial pressure...
2. Label each element with its oxidation state, use arrows to identify the reduction and oxidation, and balance the following redox reaction, which takes place under basic conditions. Please draw a box around your final balanced equation. [Note: this is a disproportionation reaction in which a species (e.g., P is oxidized and reduced.] P4 (s)PH (g) +HPO,2(aq)
2. Label each element with its oxidation state, use arrows to identify the reduction and oxidation, and balance the following redox reaction, which...
7. A low concentration of NTA has equilibrated with
PbCO3(s) at pH 7.00 in a medium having a final
HCO3- concentration of 7.50x10-4
M.
a. Determine [Pb2+].
b. Write out KT and the overall reaction for
KT.
c. What is the ratio of [Pb(NTA)- ] to
[H(NTA)2-] in this solution?
Potentially useful data: Reaction Hg 2 +2e = Hgº(s) Feste = Fe2 Cu 2 +2e = Cuº(s) 2H + 2e = H2(g) Pb2 +2e=Pbº(s) Ca*2 + 2e = Cdº(s) 1/4...
8. Sodium bicarbonate, NaHCO3, undergoes thermal decomposition according to the reaction: 2 NaHCO3 (s) + Na2CO3 (s) + CO2 (g) + H20 (g). How does the equilibrium position shift as a result of each of the following disturbances? a. 0.20 atm argon is added. b. NaHCO3 (s) is added. c. Mg(CIO)2 is added as a drying agent to remove H2O vapor. d. Dry ice (Solid CO2) is added. e. The volume of the container decreases. f. The temperature of the...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....
8. Using the Nernst equation, determine the ratio of
Hg2+ to Cu2+ at equilibrium in an
electrochemical cell in otherwise pure water, when in contact with
Hg(s) and Cu (s)
Potentially useful data: Reaction Hg 2 +2e = Hgº(s) Feste = Fe2 Cu 2 +2e = Cuº(s) 2H + 2e = H2(g) Pb2 +2e=Pbº(s) Ca*2 + 2e = Cdº(s) 1/4 O2(g) + H + = 1/2 H2O 2 02(g) + 2H+ + 2e = H,O2 1/2 NO3 + H +...
6. Given a total dissolved lead concentration of
2.0x10-5 M, a total dissolved NTA concentration of
2.0x10-2 M, and a pH of 12.3 (note extreme pH)
a. Under these conditions, what is the dominant form of NTA?
b. Write an equation for total dissolved NTA and for total
dissolved Pb. What assumptions can you make?
c. Calculate the predicted [Pb2+], considering NTA
complexation only?
d. What is the [Pb2+] as predicted by the solubility
of Pb(OH)2(s) at pH 12.3?
e....
When answering Parts a-h, consider only the molecules and ions,
Fe^2+(aq), Cd(OH)2(s), SO4^2-(aq), Al(s), I^-(aq),
and Cr2O7^2-(aq), under standard state conditions. (1 pt each)
Use standard reduction table.
a) Which of these molecules and ions are oxidizing agents?
b) Which of these molecules and ions are reducing agents?
c) List the oxidizing agents from part a in DECREASING order of
oxidizing agent strength. (strongest OA to weakest OA)
d) List the reducing agents from part b in DECREASING order of...
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