cell reaction is
H2 (g) + Cu^2+ (aq) .................> Cu (s) + 2 H+ (aq)
Q = [H+]^2 / ([Cu^2+] * P(H2))
Nernst equation is
Ecell = E0cell - 0.059 / n * log Q
Lower the H+ ion concentration leads to decrease in Q value.
As a result, Ecell increases.
option C) lower the H+ (aq) concentration is the answer.
3. For the electrochemical cell: Pt(s) | H2(1 atm) | H'(I M)I| C u2(1 M) Cu(s),...
8) An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+concentration is that of a buffer consisting of a weak acid, HA(0.115 M), mixed with its conjugate base, A-(0.192 M). The measured cell voltage is E°cell = 0.168 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = Ka =
An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+ concentration is that of a buffer consisting of a weak acid, HA(0.136 M), mixed with its conjugate base, A-(0.142 M). The measured cell voltage is E°cell = 0.196 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = _______ Ka = _______
An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+ concentration is that of a buffer consisting of a weak acid, HA(0.160 M), mixed with its conjugate base, A-(0.120 M). The measured cell voltage is E°cell = 0.228 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = Ka =
Given the electrochemical cell reaction H,(g) + PbSO,(s) 2H (a) +SO, (aq) Pb(s), predict the effect of the following changes on the observed cell voltage (increase, decrease, or no effect): a. increase in the pressure of H2 b. increase in the size of the lead electrode c. decrease in the pH of the cell electrolyte d. dissolution of Na SO, in the cell electrolyte e. decrease in the amount of PbSO f. dissolution of a small amount of NaOH in...
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
An electrochemical cell is constructed in which a Cut(1.00 M)Cu(s) half-cell is connected to an H30+(aq)H2(1 atm) half-cell with unknown Hz0+ concentration. The measured cell voltage is 0.793 V, and the Cu Cu half-cell is the cathode. What is the pH in the H3O+Hhalf-cell? The standard reduction potential for the Cu Cu half-cell is 0.522 V. pH = Submit Answer Try Another Version 3 item attempts remaining
Consider the following electrochemical cell operating at 25°C (Pt is an inert electrode): Pl(a) Cu() 1 M HNO.(4) 1 M NO, (4) 1 M H() 1 M Cu(aq) Which of the following statement(s) is (are) true when the cell operates spontaneously? (That is, when e are allowed to flow whichever way they want" to) 1. The measured voltage would be 0.603 V 2. The Pt electrode would be the anode 3. The measured voltage would be 1.277 V 4. Electrons...
5) For the electrochemical cell Ni(s) i Ni?(1 M H (1M) H (1 atm) Ps), which one of the following changes will ALWAYS cause a decrease in the cell voltage? A) Decrease the ratio of P/[Ni?') B) Increase the ratio of PH,/[N?") C) Decrease the ratio of [NiY[H] D) Increase the ratio of [Ni?'VH1 E) Increase the ratio of [H*}*/PH, Answer: ) 4) Which of the following aqueous solutions has the highest boiling point (assume 100% dissociation for all soluble...
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) | H+ (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s) given the following standard reduction potentials. Pb2+(aq) + 2 e– --> Pb(s) Edegree = –0.126 V 2 H+ (aq) + 2 e– --> H2(g) Edegree = 0.000 V (Please show the steps)
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.