Consider the galvanic cell described by (N and M are metals):
N(s)|N2+(aq)||M+(aq)|M(s)
If Eocathode = 0.585 V and Eoanode = 1.27 V, and [N2+(aq)] = 0.22 M and [M+(aq)] = 0.475 M, what is Ecell, using the Nernst equation? ____ V
Provide your response to two digits after the decimal.
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.585...
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.93 V and Eoanode = 1.814 V, and [N2+(aq)] = 0.568 M and [M+(aq)] = 0.299 M, what is Ecell, using the Nernst equation? ____ V Provide your response to two digits after the decimal.
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If E^o cathode = 0.579 V and E^o anode = 1.152 V, and [N2+(aq)] = 0.115 M and [M+(aq)] = 0.022 M, what is E cell, using the Nernst equation? ____ V Provide your response to two digits after the decimal.
Conceptual: Consider a Sn(s)|Sn2+(aq) || Cu2+(aq)|Cu(s) cell. If the Sn2+ concentration is increased, what will happen to the measured Ecell value? • Calculation, full-reaction Nernst equation: Use the full Nernst equation to calculate Ecell for the conditions described… • Easier: Ni | Ni2+(0.300 M) || Cu2+(0.002 M) | Cu • Harder: Al | Al3+(0.002 M) || Cu2+(4.00 M) | Cu • Calculation, half-reaction Nernst equation: Use the Nernst equation to calculate E at pH 3.00 and [Cl- ] = 0.0035...
Question 2 Consider a galvanic cell with the following cell notation: Cu(s)|Cu2+(0.0200 M) || Ag+ (0.0200 M)|Ag(s) a) Calculate the electrode potential at the cathode (Ecathode) b) Calculate the electrode potential at the anode (Eanode) c) Calculate the cell potential (Ecell)
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode? a) 1.03 V; b) nickel a) 1.03 V; b) silver oooo a) 0.57 V; b) nickel a) 0.57V; b) silver
5. Consider the galvanic cell, Pb(s) Pb(aq) || Cu(aq) Cu(s) What should be done to increase the cell potential (i.e., become more positive)? Be specific when stating which concentration should be increased or decreased. 6. Calculate the cell potential (Ecell) at 25°C for the cell Fe(s) / (Fe*(0.100 M) || Pd**(1.0 * 10M) | Pd(s) Given that the standard reduction potential for Fe* /Fe is -0.45 V and for Pd/Pd is +0.95 V. 8. Balance the following reduction-oxidation reaction in...
Consider the concentration cell in which the metal ion has a charge of +3, and the solution concentrations are: dilute solution = 0.007 M concentrated solution = 1.278 M What is the predicted Ecell, using the Nernst equation? ____ V Provide your response to three digits after the decimal.
A galvanic cell based on the following reactions Cu 2+ (aq) + 2e- + Cu(s) E°=0.339 V (AD + 14H(aq) + 6e-4 2Cr 3+(aq) + 7 H2O(1) Eo=1.330 V a) Write the overall cell reaction and determine its voltage. b) If the E value of the galvanic cell is 1.2 le of the galvanic cell is 1.254 V, calculate the pH of the cell when [Cu2+]=0.00010 M, Cr-0,2-1=0.00460 M, Cr3+1=1.0x102 M. The Nerst equation is E=E - (0.0592/n)logQ
III O ELECTROCHEMISTRY Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr + (aq) +3Ca (s) -- 2Cr (s) +3Ca²+ (aq) 2+ Suppose the cell is prepared with 0.699 M Cr3+ in one half-cell and 6.35 M Ca? in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 미미 X ? Check
Answer all question (a-d) thank you Consider a galvanic cell which has an Iron electrode submerged in a Fe(NO3)2 soln. and a Gold electrode submerged in a Au(NO3)3 soln. a) Find the Ecell of this cell under standard conditions: (2pts) Ans: Au3+ (aq) + 3e = Aus) ER 1.50 V + 2e = Fe(s) Er = -0.44 V Fe2+ (aq) b) Write out the balanced net reaction of this cell? (3pts) c) What is the cell potential if the concentration...