Answer is none of this
Explanation:- If you increase the concentration of one of the electrolyte solutions, you increase the number of cations and anions (depending upon which electrolyte you increase), thus increasing the voltage potential of the cell.
So that to increase potential of cell we need to increase concentration Cd 2+ ion concentration & decrease H+ ion so make difference in cell is increase & increase concentration
Consider an electrochemical cell, starting with standard state conditions, based on the following reaction. 2 H*(aq)+...
15. Consider the reaction occurring in a spontaneous electrochemical cell, starting with standard state conditions: Sn(s) + 2H*(aq) → Snº(aq) + H2(g) Which of the following actions would cause the measured cell potential, Ecell, to be greater than Eºcell, (Ecell >Ecell) A. Reducing the mass of the Sn electrode B. Increasing the mass of the Sn electrode C. Increasing the Sn?* ion concentration in the anode compartment. D. Increasing the pressure of hydrogen gas in the hydrogen cell E. Lowering...
consider the electrochemical cell 2H^+ (aq)+ Cd(s) = Cd^2+ (aq) + H2(g) Ecell°=0.40 V what would increase measured cell potential reducing H+ in hydrogen cell increasing the mass of the solid CD electrode reducing cd^2+ ion concentration increasing pressure of hydrogen gas in hydrogen cell none when 1.00kj(1000 j) of heat is added to 50.0 g of water how should the temp of the water change?
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.
Write the cell notation for an electrochemical cell consisting of an anode where Cr2+(aq) is oxidized to Cr3+(aq) at a platinum electrode and a cathode where Cd2+(aq) is reduced to Cd (s) . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.
Consider the following electrochemical cell, with a KCl(aq) salt bridge: Mn(s) | MnCl2(aq) || CdCl2(aq) | Cd(s). Identify the matching pairs below. (Use each answer exactly once.) Note that for metals, the metal refers to chemical properties and the electrode refers to physical properties, though they are the same substance. Question 8 options: 1234567 manganese ions 1234567 Cl- ions 1234567 Cd2+(aq) 1234567 Mn electrode 1234567 Mn metal 1234567 electrons 1234567 Cd electrode 1. reducing agent 2. oxidizing agent 3. transferred...
A) Write the cell notation for an electrochemical cell consisting of an anode where Mn (s) is oxidized to Mn2+(aq) and a cathode where Cd2+(aq) is reduced to Cd (s) . Assume all aqueous solutions have a concentration of 1 mol/L. B) Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+(aq) and a cathode where H+(aq) is reduced to H2(g) at a platinum electrode . Assume all aqueous solutions have...
only information present For the following electrochemical cell: Cd | Cd2+(aq) || Pb2+(aq) | Pb First, calculate Eºcell, and then calculate the value of Ecell when [Cd2+] = 4.8 M and [Pb2+1 = 8.77 x 10-6 M. +0.277 V -0.0621 V -0.107 +0.107 V +0.447 V
For the cell shown, the measured cell potential, Ecell, is -0.3707 V at 25°C. Pt(s) H(8, 0.857 atm) H+ (aq.? M) || Cd2+ (aq, 1.00 M) | Cd() The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e- H,(g) E° = 0.00 V Ca2+ (aq) + 2e Cd(s) E = -0.403 V Calculate the H* concentration.
Help! Electrochem questions: (1) An electrochemical cell consisting of a cadmium electrode immersed in a solution of 0.001M cadmium (II) nitrate, and a hydrogen electrode. The hydrogen electrode contains a solution of hydrogen cyanide. The pressure of the hydrogen gas is 1 atm. What is the concentration of the acid when there is measured a potential of 0,220V at 25 ° C. (2)A galvanic cell is composed of copper / copper ion solution (0.1M) on the one hand, and a...
Question 12 Calculate Eº for an electrochemical cell based on the following overall reaction: 2H*(aq) + Cd(s) - H2(g) + Cd2+(aq) if Erd (Hº)=0.000 V and Exped (Cd2+) = -0.402 V. 0 -0.201 V 0 -0.402 V +0.402 V +0.201 V 0.000 V