From the following list, identify the ions that are more easily reduced than H^+(aq) (a) Cu^2+(a

From the following list, identify the ions that are more...

Key Concepts

Standard Reduction Potential

The standard reduction potential is a measure of the tendency of a chemical species to gain electrons (i.e., be reduced) under standard conditions. It is expressed in volts and allows chemists to compare the relative strengths of oxidizing agents. A more positive standard reduction potential indicates a higher likelihood of a species undergoing reduction compared to one with a less positive or more negative potential.

Electrochemical Series

The electrochemical series is a ranking of chemical species based on their standard reduction potentials. This series is used to predict the direction of electron flow in redox reactions. Species higher in the series (with more positive potentials) will be reduced more easily than those lower down, enabling the prediction of which half-reaction will occur at the cathode in an electrochemical cell.

Standard Hydrogen Electrode

The Standard Hydrogen Electrode (SHE) is a reference electrode that has been assigned a potential of 0.00 V under standard conditions. It serves as the baseline for measuring the standard reduction potentials of other half-reactions. Comparing the reduction potential of a given ion to that of the SHE helps determine whether the ion is more easily reduced than hydrogen ions.

Transcript

00:01 So in this video we're supposed to identify those are those iron metal ions that are easily reduced than hydrogen.

00:11 Those that will be easily reduced, easily reduced, okay? easily reduced than hydrogen, okay? and you should know that, you should know that hydrogen is normally used as a reference, rather, there's a reference electrical potential right which which has a 0 .00 volts so this is the reference you know when you try to draw that electrical potential chart you'll have that we'll have a reference point as there as this would be hydrogen with the potential e potential right the electrode potential of 0.

01:04 0 .0 0 0 volts okay and then you'll have the negatives or rather you have positives which are also which which are on the top of the series and then negatives in the lower side of the series okay then before we answer the question we need to understand that e value we need to understand that e value of a given electrode e value of a cell electoral potential of a cell is given as e value or of reaction at the cathode, all right.

01:44 You subtract the value of the reaction found that occurs in the anode.

01:51 So that means also that that metal that will be easily reduced than hydrogen will have a positive value.

02:01 That means easily reduced, easily reduced than hydrogen will be on top of hydrogen.

02:11 So it'll be more positive than hydrogen but those are difficult to reduce will be lower than hydrogen into the difference so 0 .0 volts so that means that elector potential for a metal electrode will be negative negative here all right when referenced to standard hydrogen electrode if the metal ion is more difficult to reduce than hydrogen but the opposite is true that means electrical potential for metal electrode will be positive with reference to hydrogen if that metal is easy to reduce than hydrogen so when you write electropotentials for the list given in that scenario you have copper when you write this when you determine its electro potential okay and this copper solid e value of copper is positive as 0 .337 volts.

03:26 So also when you write for these are the reactions here for zinc...

Please give Ace some feedback