When the Pb2* concentration is 6.07x10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.148V. What is the Mg²* concentration? Pb?*(aq) + Mg(s)– Pb(s) + Mg²*(aq) Answer: M

Q: A certain metal M forms a soluble sulfate salt MSO. Suppose the left half cell of a galvanic cell…

A: Answer a:                The electrode are same in both solution at different condition it will form…

Q: What mass of Mg is produced (in grams) when a constant current of 0.752 A is passed through an…

A: Given current (I) = 0.752 A time (t) = 14.2 hours molar mass = 24.31 g/mol electrons transfer  = 2

Q: When the Cu2+ concentration is 1.02 M, the observed cell potential at 298K for an electrochemical…

A: Given: Eo (Cr3+/Cr (s)) = -0.74 V Eo (Cu2+/Cu (s)) = 0.337 VCopper act as a cathode. Chromium acts…

Q: When the Ag* concentration is 8.50×10-4 M, the observed cell potential at 298K for an…

A: The Nernst equation is given as follows, The standard cell potential of the cell is first…

Q: When the Ag* concentration is 1.17 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Pb concentration is 1.14 M, the observed cell potential at 298K for an electrochemical cell…

A:

Q: When the Pb²+ concentration is 1.68×104 M, the observed cell potential at 298K for an…

A: Introduction: The cells which can convert chemical energy to electrical energy are called…

Q: When the Cu2+ concentration is 7.81×10-4 M, the observed cell potential at 298K for an…

A:

Q: When the Pb2+ concentration is 1.21 M, the observed cell potential at 298K for an electrochemical…

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Q: TUTOR Calculate the Concentrationn of a Species Usig Cell voltage When [Cu2+] = 1.26 M, the observed…

A:

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: The EMF of the cell is calculated by below,

Q: When the Ag+ concentration is 8.96x10-4 M, the observed cell potential at 298K for an…

A: Here we are required to find the concentration of Mn2+.

Q: When the Pb2+ concentration is 1.02 M, the observed cell potential at 298K for an electrochemical…

A:

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A:

Q: When the Pb2* concentration is 1.00 M, the observed cell potential at 298K for an electrochemical…

A: It's a multiple question type and according to the guidelines of Bartleby, we are supposed to answer…

Q: When the Ag+ concentration is 5.25×10-4 M, the observed cell potential at 298K for an…

A:

Q: Ell -0.201 V for the reaction 3Pt(s)+12C1 (aq) + 2NO₁ (aq) +8H(aq) → 3PtCl(aq) + 2NO(g) + 4H₂O(1)…

A: From E°cell we can calculate individual half cell potentials.

Q: When the Cu²+ concentration is 4.32x10-4 M, the observed cell potential at 298K for an…

A: Answer: In the given cell reaction Mg is getting oxidized and Cu2+ is getting reduced, therefore Mg…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 94.68 °C with the…

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Q: When the Ag* concentration is 1.43 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Cu2+ concentration is 2.65×10-4 M, the observed cell potential at 298K for an…

A: In the given question apply Nerst equation to determine concentration of Cr+3.

Q: When the Cu²+ concentration is 9.81x10-4 M, the observed cell potential at 298K for an…

A: Given, Cu2+(aq) + Mn(s) ---> Cu(s) + Mn2+(aq) Cell potential (Ecell) = 1.428 V [Cu2+] = 9.81 ×…

Q: When the Cu²+ concentration is 1.04 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Pb2+ concentration is 1.13 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Ag+ concentration is 1.34 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Pb2+ concentration is 3.87x10-4 M, the observed cell potential at 298K for an…

A: Given-> Concentration of Pb2+ = 3.87 × 10-4 M Ecell = 1.433 V T = 298 K

Q: When the Cu2+ concentration is 1.27 M, the observed cell potential at 298K for an electrochemical…

A: Step by step solution are below

Q: When the Pb2+ concentration is 1.30 M, the observed cell potential at 298K for an electrochemical…

A: The net cell reaction :  Pb2+(aq) + Zn(s) ---> Pb(s) + Zn2+(aq)  The observed cell potential =…

Q: When the Hg2+ concentration is 6.33×10-4 M, the observed cell potential at 298K for an…

A: Interpretation : Ecell = 1.520V  Hg2+ = 6.33×10-4 M

Q: When the Ag+ concentration is 1.29 M, the observed cell potential at 298K for an electrochemical…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: When the Pb2+ concentration is 1.19 M, the observed cell potential at 298K for an electrochemical…

A: Since you have posted multiple questions as per guidelines we can answer one per session . if you…

Q: When the Ag+ concentration is 1.33 M, the observed cell potential at 298K for an electrochemical…

A: The given cell is an electrochemical cell.

Q: When the Hg** concentration is 1.45 M, the observed cell potential at 298K for an electrochemical…

A: We will use Nernst equation here. Nernst equation describes the relationship between the standard…

Q: When the Ag+ concentration is 1.29 M, the observed cell potential at 298K for an electrochemical…

A: Given: Cell reaction: 2Ag+(aq) + Zn(s)--> 2Ag(s) + Zn2+(aq) [Ag+]=1.29 M [Zn2+]=?

Q: When the Cu²+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical…

A:

Q: An unknown metal (M) is electrolyzed. It took 48.2 seconds for a current of 1.7 A to plate 0.0433 g…

A: Given, current = 1.71 A =  1.71 coulombs/sec  Time = 48.2 sec moles of e- =  1.71 x 48.2 x (1/96485)…

Q: A concentration cell is constructed using two Fe (s) electrodes each immersed in solutions of Fe, In…

A:

Q: When the Ag+ concentration is 4.05×10-4 M, the observed cell potential at 298K for an…

A: Overall cell reaction: 2Ag+(aq) + Zn(s) <---> 2Ag(s) + Zn2+(aq)

Q: When the Pb2+ concentration is 1.30 M, the observed cell potential at 298K for an electrochemical…

A: Given:  [Pb+2] = 1.30 M  Ecell = 2.344 V

Q: When the Pb2+ concentration is 1.37 M, the observed cell potential at 298K for an electrochemical…

A: The solution is given below -

Q: When the Pb²+ concentration is 1.02 M, the observed cell potential at 298 K for an cell with the…

A:

Q: When the Pb2+ concentration is 1.28 M, the observed cell potential at 298K for an electrochemical…

A: In this question, we want to determine the Concentration of Mg2+ ion in the aqueous solution,  You…

Q: When the Ag* concentration is 8.50×10-4 M, the observed cell potential at 298K for an…

A:

Q: When the Ag+ concentration is 1.24 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Ag* concentration is 1.39 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Ag+ concentration is 1.01 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Hg2+ concentration is 1.29 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Pb2+ concentration is 1.37 M, the observed cell potential at 298K for an electrochemical…

A:

Q: When the Ag* concentration is 1.33 M, the observed cell potential at 298K for an electrochemical…

A:

Q: 3 points Save Answer Consider the following reaction with vanadium and iron: 2 Fe²+ (aq) + √²+ (aq)…

A: Fe3+(aq) + e- -----> Fe2+.    E° = +0.77 V V2+.  + 2e- -----> V                E° = -0.49 V

Batteries

A battery is simply an electrochemical cell or group of cells that generate electric current. Batteries are the devices that generate current using redox reactions. These reactions proceed by the transfer of electrons. An ideal battery or cell should produce a constant voltage. A battery should actually be light in weight.