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I'm not completely certain about this but I'm convinced that an anode actually loses mass.

For example, in the cell equations for an Ag(s) cathode being dipped into an AgNO3 solution, connected to a Cu(s) anode being dipped into a Cu(NO3)2 solition,

2Ag+(aq) + 2e- -> 2Ag(s) (Cathode 1/2 reaction, reduction)

Cu(s) -> Cu2+(aq) +2e- (Anode 1/2 reaction, oxidation)

, the cathode reaction is taking the Ag+(aq) ions in the AgNO3- solution and turning them into solid silver, Ag(s). Therefore, I believe it is correct to assume that solid silver is being formed in the cathode solution.

The anode half reaction however is the opposite, taking a solid copper atom, Cu(s), and turning it into an aqueous copper cation, Cu2+(aq). This leads me to believe that the copper rod (anode) is losing mass.

So, I believe the cathode is gaining mass and the anode is losing mass.

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14y ago

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Anode rays differ from cathode rays in several aspects and their specific charge(charge/mass or e/m ratio) is an important feature. The reason lies in how anode rays are produced. Anode rays are produced when a gas at low pressure is subjected to a high voltage(10,000 Volts). Under these conditions, the atoms of the gas get ionized, i.e. they lose some electrons and thus become cations(positive ions). It is a stream of these positive ions that become 'anode rays'. However, the atomic masses of different gases are different and hence, the mass of anode ray particles varies when you use different gases in the discharge tube and hence, the charge/mass ratio also varies. Whereas, in the case of cathode rays, the cathode ray particles are nothing but electrons. Their charge and mass is constant no matter what gas you use in the discharge tube. So, their charge/mass ratio remains constant. (ANSWER BY RIZWAN FROM PAKISTAN)


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Related Questions

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During electrolysis, the mass of the anode decreases while the mass of the cathode increases. At the anode, oxidation occurs, causing the loss of mass as metal ions dissolve into the solution. Conversely, at the cathode, reduction takes place, where cations from the solution gain electrons and deposit as solid metal, thereby increasing the mass. This mass transfer is driven by the flow of electric current, facilitating the reactions at each electrode.


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