Determine Ecell (in V) at 298.15 K for a cell composed of a platinum electrode in...
Determine Ecell (in V) at 298.15 K for a cell composed of a platinum electrode in a mixture of 0.629 M Fe2+and 0.163 M Fe3+ coupled to a platinum electrode in a solution where the [H+] is 1.546 M and the partial pressure of H2 is 0.709 atm.
Homework Answers
to solve this problem we need the standats reduction potential
of Fe+3/Fe+2 which is .77 volt while standard reduction potential
of hydrogen is 0.0 volt and then applying nerst equation.
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Determine Ecell (in V) at 298.15 K for a cell
composed of a platinum electrode in...
a) Determine Ecell (in V) for a cell composed of a Ag electrode in a solution...
a) Determine Ecell (in V) for a cell composed of a Ag electrode in a solution of Ag+ coupled to a standard hydrogen electrode (SHE) under standard conditions. Report your answer to three decimal places in standard notation (i.e. 1.234 V) Ag+(aq) + e− ⇌ Ag(s) E° = 0.800 V b) Determine Ecell (in V) at 298.15 K for a cell composed of a Ag electrode in a solution of 0.528 M Ag+ coupled to a platinum electrode in a...
0.741 V You are correct. Your receipt no. is 156-8240 Previous Tries 2. Determine Ecell (in...
0.741 V You are correct. Your receipt no. is 156-8240 Previous Tries 2. Determine Ecell (in V) at 298.15 K for a cell composed of a Ti electrode in a solution of 0.372 M + coupled to a platinum electrode in a solution where the [H] is 0.984 M and the partial pressure of Hy is 1.500 atm. Report your answer to three decimal places in standard notation (I.e. 1.234 V).
this is how to question is give. A cell composed of a platinum indicator electrode and...
this is how to question is give.
A cell composed of a platinum indicator electrode and a silver-silver chloride reference electrode in a solution containing both Fe2* and Fe3+ has a cell potential of 0.699 V. If the silver-silver chloride electrode is replaced with a saturated calomel electrode (SCE), what is the new cell potential? Number 0.675
2. The electrochemical cell is comprised of a Mo electrode in a 3.87 × 10-1 M...
2. The electrochemical cell is comprised of a Mo electrode in a 3.87 × 10-1 M solution of Mo3+ (aq) coupled to a Pt electrode in a solution containing H+ (aq) where the pH of the solution is 0.16 and the partial pressure of H2(g) is 1.018 atm. The temperature of the cell is held constant at 25°C. (a)What is Ecell (in V) for the electrochemical cell? Report your answer to three decimal places in standard notation (i.e., 0.123 V)...
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of...
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2 half- cell and an H2/H half-cell under the following conditions: [Zn2] = 0.042 M [H]- 19 M partial pressure of H2 =0.37 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2 (aq) + 2e +2H (aq) + 2e1 Eo-0.76 V E 0.00 V Zn(s) H2(g)
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of...
In a test of a new reference electrode, a chemist constructs a
voltaic cell consisting of a Zn/Zn2+ half-cell and an
H2/H+ half-cell under the following
conditions: [Zn2+ ] = 0.021 M [H+ ]= 1.3 M
partial pressure of H2 = 0.32 atm. Calculate
Ecell at 298 K (enter to 3 decimal places).
Zn2+ (aq) + 2e −
⟶ Zn(s) E° = − 0.76 V
2H+ (aq) + 2e −
⟶ H2(g) E° = 0.00 V
We were unable...
Pb2+(aq) + 2e− ⇌ Pb(s) E° = -0.126 V 2H+(aq) + 2e− ⇌ H2(g) E° =...
Pb2+(aq) + 2e− ⇌ Pb(s) E° = -0.126 V 2H+(aq) + 2e− ⇌ H2(g) E° = 0.000 V E°cell (in V)= 0.126 V 2. The electrochemical cell is comprised of a Pb electrode in a 1.67 × 100 M solution of Pb2+ (aq) coupled to a Pt electrode in a solution containing H+ (aq) where the pH of the solution is 0.37 and the partial pressure of H2(g) is 0.571 atm. The temperature of the cell is held constant at...
Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential...
Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential is 0.683 V, what is the ratio of Fe2+(aq) to Fe3+(aq)? What is the ratio of these concentrations if the cell potential is 0.807 V?
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode...
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt(s)|H2(g,1atm)|H+(aq,1.0M)||Au3+(aq,?M)|Au(s). What is the concentration of Au3+ in the solution if Ecell is 1.26 V ? To what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.117 V ? (Assume that the partial pressure of hydrogen gas remains at 1 atm.) Express your answer using two decimal places.
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and...
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown [H+]. If the cell potential is 0.204 V, what is the pH of the unknown solution at 298 K? b.) An electrochemical cell is constructed in which a Cr3+(1.00 M)|Cr(s) half-cell is connected to an H3O+(aq)|H2(1 atm) half-cell with unknown H3O+ concentration. The measured cell voltage is 0.366...
0.741 V You are correct. Your receipt no. is 156-8240 Previous Tries 2. Determine Ecell (in V) at 298.15 K for a cell composed of a Ti electrode in a solution of 0.372 M + coupled to a platinum electrode in a solution where the [H] is 0.984 M and the partial pressure of Hy is 1.500 atm. Report your answer to three decimal places in standard notation (I.e. 1.234 V).
this is how to question is give.
A cell composed of a platinum indicator electrode and a silver-silver chloride reference electrode in a solution containing both Fe2* and Fe3+ has a cell potential of 0.699 V. If the silver-silver chloride electrode is replaced with a saturated calomel electrode (SCE), what is the new cell potential? Number 0.675
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2 half- cell and an H2/H half-cell under the following conditions: [Zn2] = 0.042 M [H]- 19 M partial pressure of H2 =0.37 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2 (aq) + 2e +2H (aq) + 2e1 Eo-0.76 V E 0.00 V Zn(s) H2(g)
In a test of a new reference electrode, a chemist constructs a
voltaic cell consisting of a Zn/Zn2+ half-cell and an
H2/H+ half-cell under the following
conditions: [Zn2+ ] = 0.021 M [H+ ]= 1.3 M
partial pressure of H2 = 0.32 atm. Calculate
Ecell at 298 K (enter to 3 decimal places).
Zn2+ (aq) + 2e −
⟶ Zn(s) E° = − 0.76 V
2H+ (aq) + 2e −
⟶ H2(g) E° = 0.00 V
We were unable...
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