Consider The Following Electrochemical Cell In, For Which

Electrochemical cells have two conductive electrodes, called the anode and the cathode. The anode is defined as the electrode where oxidation occurs. The cathode is the electrode where reduction takes place. Electrodes can be made from any sufficiently conductive materials, such as metals, semiconductors, graphite, and even conductive polymers.In an electrochemical cell, Q (a) Ecell is positive and EOcell (b) Ecell is negative and EOcell (c) Both E cell and are pc I from Equation 18.9, we can conclude the following: within a voltaic cell occurs under standard conditions, 0.0592 v log Q logl = 0 0.0592 v log 1 in a voltaic cell occurs under conditions in which Q < 1,Problem: If there is an electrochemical cell and Q=0.0010 and K=0.10, which is true about Ecell and Eθcell?a. Ecell is positive and Eθcell is negativeb. Ecell is negative and Eθcell is positivec. Both Ecell and Eθcell are positived.Spontaneous Voltaic Electrochemical Cells p4 Nonstandard Concentrations and Cell Potential p11 Cell Potentials p5 Electrolysis p12 E˚cell=E˚reduction + E˚oxidation ∆G˚ = -96.5nE˚cell (∆G˚ in kJ) Ecell = E˚ - [0.0592/n]log Q log K = nE˚/0.0592Given the measured cell potential, E cell, is -0.3641 V at 25 °C in the following cell, calculate the H + concentration . Pt (s) If there is an electrochemical cell and Q = 0.0010 and K = 0.10, which is true about Ecell and E°cell?a. Ecell is positive and E°cell is negativeb. Ec...

PDF (d) Both and ANSWER: (a) Since K < 1, E spontaneous

In an electrochemical cell, Q 0.10 and K = 0.0010. What can you conclude about Ecell and E? O Ecell is negative and Ec is positive. O Both Ecell and Ecellare positive. Ecoll is positive and Ellis negative. Both Ecell and Ecell are negative. Submit Request AnswerQ10. In an electrochemical cell, Q = 0.010 and K = 855. What can you conclude about Ecell and Ecell? a) Ecell is positive and Ecell is negative.In an electrochemical cell, Q= 0.10 and K= 0.0010. What can you conclude about Ecell and E∘cell? Ecell is positive and E∘cell is negative. Both Ecell and E∘cell are negative. Ecell is negative and E∘cell is positive. Both Ecell and E∘cell are positive.In an electrochemical cell, Q = 0.0010 and K = 0.10. What can you conclude about Ecell and E^o cell a. Ecell is positive and E^o cell is positive. b. Ecell is negative and E^o cell is negative. c. Both Ecell and E^o cell are positive. d. Both Ecell and E^o cell are negative.

If there is an electrochemical cell and Q=... | Clutch Prep

In an electrochemical cell, Q = 0.0010 and K = 0.10. What can you conclude about Ecell and E°cell? Since K > 1, E°cell is negative (under standard conditions, the reaction is not spontaneous). Since Q > K, Ecell is positive (the reaction is spontaneous under the nonstandard conditions of the cell).In an electrochemical cell, Q = 0.0010 and K = 0.10. What can you conclude about Ecell and E∘cell? the left half-cell will decrease in concentration; and the right half-cell will increase in concentration. Indicate what happens to the concentration of Pb2+(cathode) in each cell.In an electrochemical cell, Q=.010 and K=855. What can you conclude about Ecell and E°cell? Ecell and E°cell are both positive. A redox reaction has an E°cell=-.56 V. What can you conclude about the equilibrium constant (K) for the reaction? K<1.Question: Ifthere Is A Electrochemical Cell And Q=0.0010 And K=0.10which Is True About Ecell AndEθcell? A.) Ecell Is Positive AndEθcell Is Negativeb.) Ecell Is Negative AndEθcell Is Positivec.) Both Ecell AndEθcell Are Positived.) Both Ecell AndEθcell Are NegativeCould You Also Please Expplain Why?Problem: If there is an electrochemical cell and Q = 0.0010 and K = 0.10, which is true about Ecell and E°cell?a. Ecell is positive and E°cell is negativeb. Ecell is negative and E°cell is positivec. Both Ecell and E°cell are positived. Both Ecell and E°cell are negative

Given Data

The ratio of focus is eqQ = 0.0010 /eq. The cell consistent is eqK = 0.10 /eq.

The components to calculate the usual cellular attainable is given by way of,

eq\left( E^0 \proper)_\rmcellular = \left( \dfracRTnF \proper)\ln K /eq.

Here, eqE^0 /eq is the standard cell possible, eqR /eq is the fuel consistent, eqT /eq is the absolute temperature, eqF /eq is the Faraday constant and eqn /eq is the charge of the cell.

Substitute all the known values in the above system.

eq\startalign* \left( E^0 \proper)_\rmmobile &= \left( \dfracRTnF \proper)\ln 0.10\ &\approx - 2.303\left( \dfracRTnF \right) \finishalign* /eq

From the above calculation one can follow that the standard mobile potential is destructive.

The method to calculate the mobile possible is given via,

eq\startalign* E_\rmcell &= E^0 - \left( \dfracRTnF \proper)\ln Q\ &= \left( \dfracRTnF \right)\ln K - \left( \dfracRTnF \right)\ln Q\ &= \left( \dfracRTnF \proper)\ln \left( \dfracKQ \right) \finishalign* /eq.

Substitute all of the known values in the above formulation.

eq\startalign* E_\rmcellular &= \left( \dfracRTnF \right)\ln \left( \dfrac0.100.0010 \proper)\ &= \left( \dfracRTnF \right)\ln \left( 100 \proper)\ &= 4.605\left( \dfracRTnF \proper) \finishalign* /eq

From the above calculation one can observe that the mobile possible is certain. So we can conclude the usual cell attainable eq\left( E^0 \right)_\rmcell /eq is unfavourable and the mobile possible eqE_\rmcellular /eq is certain.

Thus, the standard cell possible eq\left( E^0 \right)_\rmcellular /eq is destructive and the cellular possible eqE_\rmcell /eq is positive.

Note- The ultimate consequence is not matching from the given choice.

Solved: 1. The Half-reaction That Should Occur At The Anod

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