SORU-13 )Boy birak - The potential created between the metal and the solution in equilibrium is called the electrode potential. I- The potential formed between metal and solution in equilibrium is called corrosion potential. III- When each metal is immersed in a 1 molar solution of its ions, the potential measured at 25 °C is called the standard electrode potential of that metal. IV. If a metal is immersed in a solution containing its ions, the metal (+) is charged with the solution (-). Which or which of the above is wrong. Yalnızi A-) I ve II B-) ve II C-) Il ve IV O O O C

SORU-13 )Boy birak - The potential created between the metal and the solution in equilibrium is called the electrode potential. I- The potential formed between metal and solution in equilibrium is called corrosion potential. III- When each metal is immersed in a 1 molar solution of its ions, the potential measured at 25 °C is called the standard electrode potential of that metal. IV. If a metal is immersed in a solution containing its ions, the metal (+) is charged with the solution (-). Which or which of the above is wrong. Yalnızi A-) I ve II B-) ve II C-) Il ve IV O O O C

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The standard hydrogen electrode (SHE) is used to produce a standard cell potential of exactly 1 V. the reference point for all standard reduction potentials. O often overlooked in measuring standard reduction potentials. used to calibrate voltmeters.
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.753 M and [Ni2+]=0.0150 M. Use the standard reduction potentials in this table. Ni2+(aq) + 2e– → Ni(s)= -0.26 Zn2+(aq) + 2e– → Zn(s)= -0.76 Zn(s)+Ni2+(aq)↽−−⇀ Zn2+(aq)+Ni(s)
7. What is the equilibrium constant, K, at 25°C for this redox reaction under standard conditions? -> 3 Ag(s) + NO¯(aq) + 4 H+(aq) → 3 Ag+(aq) +NO(g) + 2 H2O(l) A. 1.3 × 108 B. 4.8 x 1018 C. 1.9 × 10-2 D. 5.1 x 102 E. 7.6 × 10-9
Consider the following balanced equation for a redox reaction in an electrochemical cell: 3 Cd (s) + 2 NO3 (aq) + 8 H* (aq) → 3 Cd²+ (aq) + 2 NO(g) + 4H2O (1I) E°cell = 1.36 V Calculate the value of pH of the solution containing H*(aq) when the nonstandard cell potential (Ecell) is measured to be 1.12 V given the following conditions at 25 °C: [NO3] = 0.15 M; [Cd²+] = 0.46 M; PNO = 0.28 bar %3D %3D
What is electrode potential?
I need to find standard cell potential, the non-standard cell potential, using [Au^+]= 0.0015M and [Fe^3+]= 0.033M. I need to calculate Gibb's free energy and equilibrium constant, K. Is the reaction spontaneous or nonspontaneous? Are reactants or products favored at equilibrium under non-standard conditions?
Please provide the correct answer. Is pH=8.44 correct?
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which = 8.7 x 10-4 M? Ecell = b. The copper electrode is placed in a solution of unknown Cu+ |. The measured potential at 25°C is 0.223 V. What is | Cu²+ |? (Assume Cu²+ is reduced.) [C*] = Cu² 2+ M
_____ H3PO4 + _____ KOH ----> _____ K3PO4 + _____ H2O
Clinical Chemistry The concentration of Na+ ions in red blood cells (8.00 mM) and in the surrounding plasma (143.0 mM) are quite different. Calculate the electrochemical potential (emf) across the cell membrane as a result of this concentration gradient (Body temperature is 37.0°C) Calculate the osmotic pressure exerted by the plasma at body temperature (37.0°C).
The following half-cells are on the left and coupled with the standard hydrogen electrode on the right to form a galvanic Calculate the cell potential. If the cell were shorted, indicate whether the electrodes shown would act as an anode or a cathode. a. Cu Cu²+ (0.0567 M), (Cu²+/Cu = 0.337 V) V Potential = b. Cu | Cul (sat'd), KI (0.0939 M), (ECul/Cu = -0.185 V) Potential = V 3+ c. Pt | Fe³+ (0.160 M), Fe²+ (0.08340 M), (E Potential = V Fe³+/Fe²+ = = 0.771 V)
Cu = reduction potential of +0.52. Mg is in pic. Thanks