Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.084...
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.084 V and Eoanode = 1.131 V, and [N2+(aq)] = 0.903 M and [M+(aq)] = 0.819 M, what is Ecell, using the Nernst equation? ____ V Provide your response to two digits after the decimal.
keep in mind, for Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.915 V and Eoanode = 1.371 V, and [N2+(aq)] = 0.008 M and [M+(aq)] = 0.855 M, what is Ecell, using the Nernst equation? , the answer is -0.398
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Consider the galvanic cell described by (N and M are metals):
N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.084...
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 = 0.585 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.
Question 1 1 pts Consider the galvanic cell described by (N and Mare metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eºcathode = 0.585 V and Eanode = 1.27 V, and [N2+(aq)] = 0.22 M...
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 Eoano...
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 =...
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...
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...
5. Consider the galvanic cell, Pb(s) Pb(aq) || Cu(aq) Cu(s) What should be done to increase...
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...
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a)...
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
Answer all question (a-d) thank you Consider a galvanic cell which has an Iron electrode submerged...
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...
A galvanic cell based on the following reactions Cu 2+ (aq) + 2e- + Cu(s) E°=0.339...
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
Consider a galvanic cell where one compartment has Br2 (aq) at a concentration of 0.50 M and Br ̄ at a concentration of...
Consider a galvanic cell where one compartment has Br2 (aq) at a concentration of 0.50 M and Br ̄ at a concentration of 0.10 M with a platinum electrode and the second compartment has Cr3+ at a concentration of 0.20 M and a Cr electrode. Use the following reduction potentials to answer the questions: Cr3+ (aq) + e ̄→Cr(s) εo = - 0.73 V Br2(aq) + 2e ̄→2Br ̄ (aq) εo =1.09V a. What is the standard cell potential for...
pleas help me with lab assament Multimeter Consider a galvanic cell consisting of the following two...
pleas help me with lab assament
Multimeter Consider a galvanic cell consisting of the following two redox couples: Ag+(0.010 M) + e-→ Ag(s) Eo = +0.80 V oi a. Write the equation for the half-reaction occurring at the Salt bridge C (0.010 M) Ag (0.010AM b. Write the equation for the half-reaction occurring at the anode. Cr Ag c. Write the equation for the cell reaction. d. What is the standard cell potential, Eelli for the cell? e. Realizing the...
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.
Question 1 1 pts Consider the galvanic cell described by (N and Mare metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eºcathode = 0.585 V and Eanode = 1.27 V, and [N2+(aq)] = 0.22 M...
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...
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
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...
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
pleas help me with lab assament
Multimeter Consider a galvanic cell consisting of the following two redox couples: Ag+(0.010 M) + e-→ Ag(s) Eo = +0.80 V oi a. Write the equation for the half-reaction occurring at the Salt bridge C (0.010 M) Ag (0.010AM b. Write the equation for the half-reaction occurring at the anode. Cr Ag c. Write the equation for the cell reaction. d. What is the standard cell potential, Eelli for the cell? e. Realizing the...
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