Question

In: Chemistry

Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 89 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.110 M...

Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 89 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.110 M .

Part A:

What is the value for the reaction quotient, Q, for the cell?

Part B:

What is the value for the temperature, T, in kelvins?

Part C:

What is the value for n?

Part D:

Calculate the standard cell potential for

Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)

Solutions

Expert Solution

Mg(s) ----------------> Mg^2+ (aq) + 2e^- E0 = 2.38v

Fe^2+ (aq) + 2e^- ------> Fe(s) E0 = -0.41v

-----------------------------------------------------------------------------------

Mg(s) + Fe^2+ (aq) -----> Mg^2+ (aq) + Fe(s) E0cell = 1.97v

the standard cell potential for 1.97v

n = 2

T = 89+273 = 362K

Mg(s) + Fe^2+ (aq) -----> Mg^2+ (aq) + Fe(s)

[Fe2+]= 3.00 M and [Mg2+]= 0.110 M .

Q = [Mg^2+]/[Fe^2+]

= 0.11/3 = 0.0366

Ecell = E0cell - 0.0592/n logQ

= 1.97 -0.0592/2 log0.0366

= 1.97 -0.0296*-1.4365 = 2.0125v

part-A

Mg(s) + Fe^2+ (aq) -----> Mg^2+ (aq) + Fe(s)

[Fe2+]= 3.00 M and [Mg2+]= 0.110 M .

Q = [Mg^2+]/[Fe^2+]

= 0.11/3 = 0.0366

part-B

T = 89+273 = 362K

part-C

n = 2 electrons are involve in the reaction

part-D

Mg(s) ----------------> Mg^2+ (aq) + 2e^- E0 = 2.38v

Fe^2+ (aq) + 2e^- ------> Fe(s) E0 = -0.41v

-----------------------------------------------------------------------------------

Mg(s) + Fe^2+ (aq) -----> Mg^2+ (aq) + Fe(s) E0cell = 1.97v

the standard cell potential for 1.97v

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 73 ∘C , where [Fe2+]= 3.70 M and [Mg2+]= 0.310 M...

Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 73 ∘C , where [Fe2+]= 3.70 M and [Mg2+]= 0.310 M . What is the value for the reaction quotient, Q, for the cell? What is the value for the temperature, T, in kelvins? What is the value for n? Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)

Consider an electrochemical cell based on the following overall reaction, Fe(s) + 2Ag+(aq)  Fe2+(aq) +...

Consider an electrochemical cell based on the following overall reaction, Fe(s) + 2Ag+(aq)  Fe2+(aq) + 2Ag(s) Fe2+(aq) + 2e– Fe(s), ℰ° = –0.44 V Ag+(aq) + e– Ag, ℰ° = 0.80 V Calculate the cell potential (in V) for this reaction at 25oC when the concentration of Ag+ ions is 0.050 M and the concentration of Fe2+ ions is 1.50 M. a. +1.32 V b. +1.50 V c. +1.20 V d. -1.32 V e. -1.20 V

Calculate the Kc for the following reaction at 25 °C: Mg(s) + Pb2+(aq)?Mg2+(aq) + Pb(s) Kc...

Calculate the Kc for the following reaction at 25 °C: Mg(s) + Pb2+(aq)?Mg2+(aq) + Pb(s) Kc = × 10 Enter your answer in scientific notation.

Derive a balanced equation for the reaction occurring in the cell: Fe(s)|Fe2+(aq)||Fe3+(aq),Fe2+(aq)|Pt(s) a.) If E?cell =...

Derive a balanced equation for the reaction occurring in the cell: Fe(s)|Fe2+(aq)||Fe3+(aq),Fe2+(aq)|Pt(s) a.) If E?cell = 1.21 V, calculate ?G? for the reaction. b.) If E?cell=1.21V, calculate the equilibrium constant for the reaction. c.) Use the Nernst equation to determine the potential for the cell: Fe(s)|Fe2+(aq,1.0�10-3M)||Fe3+(aq,1.0�10-3M),Fe2+(aq,0.10M)|Pt(s)

Suppose you construct the following galvanic cell: Fe(s)|Fe2+(aq)||NAD+(aq)|NADH(aq) Fe2+ + 2e- → Fe Eo = -0.44V...

Suppose you construct the following galvanic cell: Fe(s)|Fe2+(aq)||NAD+(aq)|NADH(aq) Fe2+ + 2e- → Fe Eo = -0.44V NAD+ + 2e- + 2H+ → NADH + H+ Eo' = -0.320V (note the different standard states) A) Will the cell generate current at biochemical standard state? At chemical standard state? At T = 4 oC, pH = 7? At T = 97 oC, pH = 7? Justify your answers. B) How many protons can be moved across a membrane from pH 7.5 to...

Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If...

Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.236 volts, what is the pH of the hydrogen electrode? A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ()= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.202 V, what is the pH of the unknown solution at 298...

A galvanic cell Fe(s)|Fe2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Fe electrode that weighs...

A galvanic cell Fe(s)|Fe2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Fe electrode that weighs 35.6 g and a Pbelectrode immersed in 510 mL of 1.00 M Pb2+(aq) solution. A steady current of 0.0672 A is drawn from the cell as the electrons move from the Fe electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? -------- s...

Calculate the Eocell for: Fe(s) + Br2(g) → Fe2+(aq) +Br-(aq) ; is this electrolytic or voltaic?...

Calculate the Eocell for: Fe(s) + Br2(g) → Fe2+(aq) +Br-(aq) ; is this electrolytic or voltaic? A. -1.52V ; voltaic B. 1.52V ; electrolytic C. -1.52V ; electrolytic D. 1.52V ; voltaic

For the voltaic cell, Cr(s) │ Cr3+ (aq, 0.24 M) ││ Fe2+ (aq, (?) M) │...

For the voltaic cell, Cr(s) │ Cr3+ (aq, 0.24 M) ││ Fe2+ (aq, (?) M) │ Fe(s) , Ecell is 0.33 V. Calculate the concentration of Fe2+ (M). Reduction potential for Cr3+(aq)/Cr(s) is -0.74 V, Fe2+(aq)/Fe(s) is -0.44 V. Enter number to 2 decimal places.

Co(s) → Co2+(aq) + 2e Fe2+(aq) + 2e-→ Fe(s) b) Calculate the standard cell potential for...

Co(s) → Co2+(aq) + 2e Fe2+(aq) + 2e-→ Fe(s) b) Calculate the standard cell potential for this voltaic cell. c) Calculate the cell potential for this voltaic cell at 298 K if it is constructed using solutions of 0.14 M Co(NO3)2 and 0.27 M Fe(NO3)2. d) When looking at the magnitude of this potential, what can be concluded about the electrochemical cell?

Subjects