Chemistry, 19.07.2019 20:30 photon22

Agalvanic cell has an x electrode with x 2 plus ions in the left beaker and a y electrode with y 2 plus ions in the right beaker. a salt bridge connects the two halves. consider a galvanic (voltaic) cell that has the generic metals x and y as electrodes. if x is more reactive than y (that is, x more readily reacts to form a cation than y does), classify the descriptions by whether they apply to the x or y electrode.

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Answer from: tiwaribianca475

The anode is X and the cathode is Y

Further explanation

Voltaic cells or also called galvanic cells are electrochemical cells that produce electrical energy due to redoxs reactions / chemical reactions.

Electric current is generated due to the flow of electrons from the anode that undergoes an oxidation reaction to the cathode which has a reduction reaction in the circuit of an outer wire circuit

The parts of a voltaic cell are:

Cathode : reduction occurs, a positive poleAnode: oxidation occurs, a negative poleElectrolytes: an electrically conductive solution on both electrodesConductor wire: the link between the cathode and the anodeSalt bridge: as neutralizing anions and excess cations of electrolyte solution (supplying anions to the anode and cations to the cathode; for example KNO₃ solution)

Cell potential (E °) is the potential difference between the two electrodes in an electrochemical cell.

Electric current moves from a high potential pole to a low potential, so the cell potential is the difference between an electrode that has a high electrode potential (cathode) and an electrode that has a low electrode potential (anode)

E ° cell = E ° cathode -E ° anode

or:

E ° cell = E ° reduction-E ° oxidation

The cathode has more positive E °, and anode has smaller (negative) E °

Potential positive reactions indicate reactions take place spontaneously

The metal activity series, called the Volta series, shows metal reactivity in redox reactions

The order is:

Li K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb H Cu Hg Ag Pt Au

The metal element with a standard electrode potential is smaller on the left, while the metal with a larger electrode potential on the right.

From left to right: the reactivity of the metal decreases (reactive = easier to release electrons), the reducing power (reducing agent) decreases, the oxidizing power (oxidizing) increases

So the metal element on the left can push/reduce the metal on the right so that the reaction is spontaneous

While the metal element on the right is not able to oxidize the left metal

If x is more reactive than y (that is, x is more readily reacts to the form than y does),

So that X easily releases electrons, oxidation reactions occur,

X ----> X²⁺ + 2e⁻, and

Y reduction reactions occur,

Y²⁺ + 2e⁻ ---> Y

So the anode is X and the cathode is Y

The cell : (left anode, right cathode)

X | X²⁺ || Y²⁺ | Y

E cell = E ° Y - E ° X

In the voltaic array, the position of the element X is to the left of the element Y