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 solution where the [H+] is 1.870 M and the partial pressure of H2 is 0.426 atm. Report your answer to three decimal places in standard notation (i.e. 1.234 V).
a) Determine Ecell (in V) for a cell composed of a Ag electrode in a solution...
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).
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.
7.An electrochemical cell consists of a Mg electrode in a solution of 0.548 M Mg+ coupled to a Pd electrode in a solution of 0.438 M Pd2+ , all held at 20.1 °C. Mg+(aq) + e− ⇌ Mg(s) E° = -2.700 V Pd2+(aq) + 2e− ⇌ Pd(s) E° = 0.951 V 1. Determine Ecell (in V). Report your answer to three decimal places in standard notation (i.e. 1.234 V). Tries 0/3 2. Determine ΔG (in kJ). Report your answer to three significant...
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)...
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...
OV L'0000 V Whats Report you to two three decalcesidad (b) the electrochemical comprised of all electrode in a 7.86 10 solution of led to a 15 marks the of the col competent on the is incredo answer to three decimal places in standard m one, 123V). Tit(aq) + e- TH(s) E = -0.336 V 2H(aq) + 2e- H2() E = 0.000 V (a) [1 mark] What is Eºcell (in V)? Report your answer to two three decimal places in...
A voltaic cell represented by the following cell diagram has Ecell= 1.409 V . Zn(s)|Zn2+(1.00M)||Ag+(saturated Ag2X)|Ag(s) What must be the Ksp of Ag2X? Use the following standard electrode potentials: Zn2+(aq) + 2e- →Zn(s) E° = -0.764 V Ag+(aq) + e- →Ag(s) E° = 0.799 V To enter your answer, multiply your Ksp by 1x109 then enter it to 2 decimal places.
A galvanic (voltaic) cell consists of an electrode composed of magnesium in a 1.0 M magnesium ion solution and another electrode composed of copper in a 1.0 M copper(I) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. Ecell = | 2.46
Use the reduction potentials and the unbalanced chemical equation below to answer the following questions: Mn2+ (aq) + Ag+ (aq) → Mn (s) + Ag2+ (aq) Half-cell reaction / E° (V) Mn2+(aq) + 2e− ⇌ Mn(s) / -1.185 Ag2+(aq) + e− ⇌ Ag+(aq) / 1.980 a) Determine E°cell (in V). Report your answer to three decimal places in standard notation (i.e. 1.234 V) b) Determine ΔG° (in kJ/mol). Report your answer to three significant figures in scientific notation (i.e. 1.23e4...
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