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rite reaction quotients for each of the following. For gases use pressure, P, and for solution...
1. Determine if each of the following reactions is a redox reaction, or is not a...
1. Determine if each of the following reactions is a redox reaction, or is not a redox reaction. a. C4H8 (g) + O2 + H20 (g) + CO2 (g) b. HCl (aq) + NaOH (aq) → H20 (1) + NaCl (aq) c. Fe2O3 + H2 → Fe + H2O d. Cu (s) + HNO3 (aq) → Cu(NO3)2 (aq) + NO2 (g) + H20 (1) e. CzHe(g) + 5 O2 (g) → 3 CO2 (g) + 4 H20 (g)
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are...
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are A = 0.076 M B = 0.829 M If K = 3.32, find the concentration of C and report it in M units. B.) Cu (s) + 2 Ag+ ⇋ Cu2+ (aq+) + 2 Ag(s) K = 7.88 x 104 PbCl2 (s) ⇋ Pb2+ (aq) + 2 Cl- (aq) K = 2.4 x 10-4 AgI (s) ⇋ Ag+ (aq) + I- (aq) K =...
What type of reaction is occurring in each step? Give a brief description for your choice....
What type of reaction is occurring in each step? Give a brief
description for your choice. Provide a complete balanced reaction
equations for the two redox reactions. Indicate which species is
being oxidize and which is being reduced in each case.
PART A: Cu (s) + 2 NO3- (aq) + 4 H+ (aq) + 4 H20 (1) → [Cu(H20)6]2+ (aq) + 2 NO2(g) (1) PART B: [Cu(H20)6]2+ (aq) + 2 H20 - (aq) + Cu(OH)2 (5) + 6 H20 (1)...
8 The Following reaction is classified as: 2HCl(aq) + Ba(OH)2(aq) → BaCl(aq) + 2 H20(0) b)...
8 The Following reaction is classified as: 2HCl(aq) + Ba(OH)2(aq) → BaCl(aq) + 2 H20(0) b) precipitation reaction oxidation-reduction reaction d) acid-base neutralization reaction 9. c) single replacement What is the volume of 0.1220 M HNO, solution required to completely neutralize 17.50 ml of 0.1211M NAOH? Reaction is: HNO, (aq) + NaOH(aq) -NaNO, (aq) + H:0 (aq) a) 17.37 ml b) 16.31 ml. c) 15.39 ml. d) 17.84 mL 10. Which one of the following reactions is the reduction reaction?...
For each reaction below, balance the following reactions and indicate the species that has been oxidized...
For each reaction below,
balance the following reactions and indicate the species that has
been oxidized and the species that has been reduced: Copy and paste
the table below, to complete the chart.
For each reaction below, balance the following reactions and indicate the species that has been oxidized and the species that has been reduced: Copy and paste the table below, to complete the chart. Reaction Species Oxidized Species Reduced Cl2 (g) + (aq) → 12 (s) + Cl(aq)...
use the example to answer 8,9,10&11 Here's an example: Balance the following redox reaction, which occurs...
use the example to answer
8,9,10&11
Here's an example: Balance the following redox reaction, which occurs in acidic solution: Fe (aq)+ MnO4'(aq) -Fe (aq) + Mn (aq) Solution: +2 +7 +3 Step 1) +2 Fe2 (aq)+ MnOa (aq) Fe(aq) + Mn2 (aq) Fe (aq) MnO4 (aq) Mn2 (aq) 1 Fe on each side; 1 Mn on each side; no adjustment necessary Fe2 (aq) Fe 3'(aq) + e 5 e + MnO4(aq) Fe (aq) Fe (aq) + e (2+ on each...
help with these please Use the References to access important values if needed for this question....
help with these please
Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2 concentration is 9.24x104 M and the Cr3 concentration is 1.47 M ? 3Cu2 (aq)+2Cr(s)3Cu(s) + 2Cr (aq) V Answer: The cell reaction as written above is spontaneous for the concentrations given: What is the binding energy in kJ/mol nucleons for silver-107? kJ/mol...
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown...
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
Use the following half-reactions to write 3 spontaneous reactions, calculate E°cell for each reaction, what is...
Use the following half-reactions to write 3 spontaneous
reactions, calculate E°cell for each reaction, what is
the n number (number of electrons transferred).
Au+ (aq) + e− → Au
(s) E° = 1.69
V
N2O (g) + 2H+ (aq) + 2 e− →
N2 (g) + H2O (l) E° =
1.77 V
Cr3+ (aq) + 3 e− → Cr
(s) E° = -0.74 V
Question 7 0.36 pts Use the following half-reactions to write 3 spontaneous reactions, calculate Eºcell for...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO3- (aq)...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO3- (aq) + N2O (g) (ii) (acid solution) Fe042- (aq) + Fe3+ (aq) (iii) (base solution) Fe203 () → Fe(OH)2 (S) (iv) (base solution) Cu20 (s) + Cu(OH)2 (S) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
1. Determine if each of the following reactions is a redox reaction, or is not a redox reaction. a. C4H8 (g) + O2 + H20 (g) + CO2 (g) b. HCl (aq) + NaOH (aq) → H20 (1) + NaCl (aq) c. Fe2O3 + H2 → Fe + H2O d. Cu (s) + HNO3 (aq) → Cu(NO3)2 (aq) + NO2 (g) + H20 (1) e. CzHe(g) + 5 O2 (g) → 3 CO2 (g) + 4 H20 (g)
What type of reaction is occurring in each step? Give a brief
description for your choice. Provide a complete balanced reaction
equations for the two redox reactions. Indicate which species is
being oxidize and which is being reduced in each case.
PART A: Cu (s) + 2 NO3- (aq) + 4 H+ (aq) + 4 H20 (1) → [Cu(H20)6]2+ (aq) + 2 NO2(g) (1) PART B: [Cu(H20)6]2+ (aq) + 2 H20 - (aq) + Cu(OH)2 (5) + 6 H20 (1)...
8 The Following reaction is classified as: 2HCl(aq) + Ba(OH)2(aq) → BaCl(aq) + 2 H20(0) b) precipitation reaction oxidation-reduction reaction d) acid-base neutralization reaction 9. c) single replacement What is the volume of 0.1220 M HNO, solution required to completely neutralize 17.50 ml of 0.1211M NAOH? Reaction is: HNO, (aq) + NaOH(aq) -NaNO, (aq) + H:0 (aq) a) 17.37 ml b) 16.31 ml. c) 15.39 ml. d) 17.84 mL 10. Which one of the following reactions is the reduction reaction?...
For each reaction below,
balance the following reactions and indicate the species that has
been oxidized and the species that has been reduced: Copy and paste
the table below, to complete the chart.
For each reaction below, balance the following reactions and indicate the species that has been oxidized and the species that has been reduced: Copy and paste the table below, to complete the chart. Reaction Species Oxidized Species Reduced Cl2 (g) + (aq) → 12 (s) + Cl(aq)...
use the example to answer
8,9,10&11
Here's an example: Balance the following redox reaction, which occurs in acidic solution: Fe (aq)+ MnO4'(aq) -Fe (aq) + Mn (aq) Solution: +2 +7 +3 Step 1) +2 Fe2 (aq)+ MnOa (aq) Fe(aq) + Mn2 (aq) Fe (aq) MnO4 (aq) Mn2 (aq) 1 Fe on each side; 1 Mn on each side; no adjustment necessary Fe2 (aq) Fe 3'(aq) + e 5 e + MnO4(aq) Fe (aq) Fe (aq) + e (2+ on each...
help with these please
Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2 concentration is 9.24x104 M and the Cr3 concentration is 1.47 M ? 3Cu2 (aq)+2Cr(s)3Cu(s) + 2Cr (aq) V Answer: The cell reaction as written above is spontaneous for the concentrations given: What is the binding energy in kJ/mol nucleons for silver-107? kJ/mol...
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
Use the following half-reactions to write 3 spontaneous
reactions, calculate E°cell for each reaction, what is
the n number (number of electrons transferred).
Au+ (aq) + e− → Au
(s) E° = 1.69
V
N2O (g) + 2H+ (aq) + 2 e− →
N2 (g) + H2O (l) E° =
1.77 V
Cr3+ (aq) + 3 e− → Cr
(s) E° = -0.74 V
Question 7 0.36 pts Use the following half-reactions to write 3 spontaneous reactions, calculate Eºcell for...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO3- (aq) + N2O (g) (ii) (acid solution) Fe042- (aq) + Fe3+ (aq) (iii) (base solution) Fe203 () → Fe(OH)2 (S) (iv) (base solution) Cu20 (s) + Cu(OH)2 (S) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
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